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<span>Sulphides</span> </div> </a> <button aria-controls="toc-Sulphides-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Sulphides subsection</span> </button> <ul id="toc-Sulphides-sublist" class="vector-toc-list"> <li id="toc-Sodium_Nitroprusside" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Sodium_Nitroprusside"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.1</span> <span>Sodium Nitroprusside</span> </div> </a> <ul id="toc-Sodium_Nitroprusside-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Silver_Nitrate" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Silver_Nitrate"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.2</span> <span>Silver Nitrate</span> </div> </a> <ul id="toc-Silver_Nitrate-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Lead_Ethanoate" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Lead_Ethanoate"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.3</span> <span>Lead Ethanoate</span> </div> </a> <ul id="toc-Lead_Ethanoate-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-H2S" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#H2S"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.4</span> <span>H<sub>2</sub>S</span> </div> </a> <ul id="toc-H2S-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-The_nitrite_ion" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#The_nitrite_ion"> <div class="vector-toc-text"> <span class="vector-toc-numb">2</span> <span>The nitrite ion</span> </div> </a> <button aria-controls="toc-The_nitrite_ion-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle The nitrite ion subsection</span> </button> <ul id="toc-The_nitrite_ion-sublist" class="vector-toc-list"> <li id="toc-I3-" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#I3-"> <div class="vector-toc-text"> <span class="vector-toc-numb">2.1</span> <span>I<sub>3</sub>-</span> </div> </a> <ul id="toc-I3--sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Lead/Silver_Nitrates" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Lead/Silver_Nitrates"> <div class="vector-toc-text"> <span class="vector-toc-numb">2.2</span> <span>Lead/Silver Nitrates</span> </div> </a> <ul id="toc-Lead/Silver_Nitrates-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-The_cyanide_ions" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#The_cyanide_ions"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>The cyanide ions</span> </div> </a> <button aria-controls="toc-The_cyanide_ions-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle The cyanide ions subsection</span> </button> <ul id="toc-The_cyanide_ions-sublist" class="vector-toc-list"> <li id="toc-Ferric_ions" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Ferric_ions"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.1</span> <span>Ferric ions</span> </div> </a> <ul id="toc-Ferric_ions-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Metallic_copper" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Metallic_copper"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.2</span> <span>Metallic copper</span> </div> </a> <ul id="toc-Metallic_copper-sublist" class="vector-toc-list"> <li id="toc-Note_on_the_tetracyano_complex_of_copper" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Note_on_the_tetracyano_complex_of_copper"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.2.1</span> <span>Note on the tetracyano complex of copper</span> </div> </a> <ul id="toc-Note_on_the_tetracyano_complex_of_copper-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> </ul> </li> <li id="toc-The_hypochlorite_ion" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#The_hypochlorite_ion"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>The hypochlorite ion</span> </div> </a> <ul id="toc-The_hypochlorite_ion-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-The_azide_ion" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#The_azide_ion"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>The azide ion</span> </div> </a> <ul id="toc-The_azide_ion-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-The_acetate_ion" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#The_acetate_ion"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>The acetate ion</span> </div> </a> <button aria-controls="toc-The_acetate_ion-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle The acetate ion subsection</span> </button> <ul id="toc-The_acetate_ion-sublist" class="vector-toc-list"> <li id="toc-Acidification" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Acidification"> <div class="vector-toc-text"> <span class="vector-toc-numb">6.1</span> <span>Acidification</span> </div> </a> <ul id="toc-Acidification-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Esterification" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Esterification"> <div class="vector-toc-text"> <span class="vector-toc-numb">6.2</span> <span>Esterification</span> </div> </a> <ul id="toc-Esterification-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Ferric_Chloride" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Ferric_Chloride"> <div class="vector-toc-text"> <span class="vector-toc-numb">6.3</span> <span>Ferric Chloride</span> </div> </a> <ul id="toc-Ferric_Chloride-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Thiosulphates" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Thiosulphates"> <div class="vector-toc-text"> <span class="vector-toc-numb">7</span> <span>Thiosulphates</span> </div> </a> <button aria-controls="toc-Thiosulphates-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Thiosulphates subsection</span> </button> <ul id="toc-Thiosulphates-sublist" class="vector-toc-list"> <li id="toc-Hydronium_ions" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Hydronium_ions"> <div class="vector-toc-text"> <span class="vector-toc-numb">7.1</span> <span>Hydronium ions</span> </div> </a> <ul id="toc-Hydronium_ions-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Ferric_ions_2" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Ferric_ions_2"> <div class="vector-toc-text"> <span class="vector-toc-numb">7.2</span> <span>Ferric ions</span> </div> </a> <ul id="toc-Ferric_ions_2-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Copper_Sulphate" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Copper_Sulphate"> <div class="vector-toc-text"> <span class="vector-toc-numb">7.3</span> <span>Copper Sulphate</span> </div> </a> <ul id="toc-Copper_Sulphate-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Silver_Nitrate_2" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Silver_Nitrate_2"> <div class="vector-toc-text"> <span class="vector-toc-numb">7.4</span> <span>Silver Nitrate</span> </div> </a> <ul id="toc-Silver_Nitrate_2-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Thiocyanate_ions" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Thiocyanate_ions"> <div class="vector-toc-text"> <span class="vector-toc-numb">8</span> <span>Thiocyanate ions</span> </div> </a> <button aria-controls="toc-Thiocyanate_ions-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Thiocyanate ions subsection</span> </button> <ul id="toc-Thiocyanate_ions-sublist" class="vector-toc-list"> <li id="toc-Ferricthiocyanate" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Ferricthiocyanate"> <div class="vector-toc-text"> <span class="vector-toc-numb">8.1</span> <span>Ferricthiocyanate</span> </div> </a> <ul id="toc-Ferricthiocyanate-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Vogel's_test" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Vogel's_test"> <div class="vector-toc-text"> <span class="vector-toc-numb">8.2</span> <span>Vogel's test</span> </div> </a> <ul id="toc-Vogel's_test-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Fluorides" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Fluorides"> <div class="vector-toc-text"> <span class="vector-toc-numb">9</span> <span>Fluorides</span> </div> </a> <button aria-controls="toc-Fluorides-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Fluorides subsection</span> </button> <ul id="toc-Fluorides-sublist" class="vector-toc-list"> <li id="toc-Evolution_of_HF" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Evolution_of_HF"> <div class="vector-toc-text"> <span class="vector-toc-numb">9.1</span> <span>Evolution of HF</span> </div> </a> <ul id="toc-Evolution_of_HF-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Oxidation_of_fluorides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Oxidation_of_fluorides"> <div class="vector-toc-text"> <span class="vector-toc-numb">9.2</span> <span>Oxidation of fluorides</span> </div> </a> <ul id="toc-Oxidation_of_fluorides-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Chlorides" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Chlorides"> <div class="vector-toc-text"> <span class="vector-toc-numb">10</span> <span>Chlorides</span> </div> </a> <button aria-controls="toc-Chlorides-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Chlorides subsection</span> </button> <ul id="toc-Chlorides-sublist" class="vector-toc-list"> <li id="toc-Conc._H2SO4" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Conc._H2SO4"> <div class="vector-toc-text"> <span class="vector-toc-numb">10.1</span> <span>Conc. H<sub>2</sub>SO<sub>4</sub></span> </div> </a> <ul id="toc-Conc._H2SO4-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-The_Silver_Nitrate_test" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#The_Silver_Nitrate_test"> <div class="vector-toc-text"> <span class="vector-toc-numb">10.2</span> <span>The Silver Nitrate test</span> </div> </a> <ul id="toc-The_Silver_Nitrate_test-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-The_Chromyl_Chloride_test" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#The_Chromyl_Chloride_test"> <div class="vector-toc-text"> <span class="vector-toc-numb">10.3</span> <span>The Chromyl Chloride test</span> </div> </a> <ul id="toc-The_Chromyl_Chloride_test-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Bromides/Iodides" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Bromides/Iodides"> <div class="vector-toc-text"> <span class="vector-toc-numb">11</span> <span>Bromides/Iodides</span> </div> </a> <button aria-controls="toc-Bromides/Iodides-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Bromides/Iodides subsection</span> </button> <ul id="toc-Bromides/Iodides-sublist" class="vector-toc-list"> <li id="toc-Conc._H2SO4_2" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Conc._H2SO4_2"> <div class="vector-toc-text"> <span class="vector-toc-numb">11.1</span> <span>Conc. H2SO4</span> </div> </a> <ul id="toc-Conc._H2SO4_2-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Silver_nitrate_solution" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Silver_nitrate_solution"> <div class="vector-toc-text"> <span class="vector-toc-numb">11.2</span> <span>Silver nitrate solution</span> </div> </a> <ul id="toc-Silver_nitrate_solution-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-The_Chloroform_test" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#The_Chloroform_test"> <div class="vector-toc-text"> <span class="vector-toc-numb">11.3</span> <span>The Chloroform test</span> </div> </a> <ul id="toc-The_Chloroform_test-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Oxalate_ions" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Oxalate_ions"> <div class="vector-toc-text"> <span class="vector-toc-numb">12</span> <span>Oxalate ions</span> </div> </a> <button aria-controls="toc-Oxalate_ions-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Oxalate ions subsection</span> </button> <ul id="toc-Oxalate_ions-sublist" class="vector-toc-list"> <li id="toc-Conc._H2SO4_3" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Conc._H2SO4_3"> <div class="vector-toc-text"> <span class="vector-toc-numb">12.1</span> <span>Conc. H<sub>2</sub>SO<sub>4</sub></span> </div> </a> <ul id="toc-Conc._H2SO4_3-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Acidified_Potassium_Permanaganate_solution" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Acidified_Potassium_Permanaganate_solution"> <div class="vector-toc-text"> <span class="vector-toc-numb">12.2</span> <span>Acidified Potassium Permanaganate solution</span> </div> </a> <ul id="toc-Acidified_Potassium_Permanaganate_solution-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Calcium_chloride_solution" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Calcium_chloride_solution"> <div class="vector-toc-text"> <span class="vector-toc-numb">12.3</span> <span>Calcium chloride solution</span> </div> </a> <ul id="toc-Calcium_chloride_solution-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Nitrates" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Nitrates"> <div class="vector-toc-text"> <span class="vector-toc-numb">13</span> <span>Nitrates</span> </div> </a> <button aria-controls="toc-Nitrates-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Nitrates subsection</span> </button> <ul id="toc-Nitrates-sublist" class="vector-toc-list"> <li id="toc-Decomposition_by_Heat_or_Strong_Acid" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Decomposition_by_Heat_or_Strong_Acid"> <div class="vector-toc-text"> <span class="vector-toc-numb">13.1</span> <span>Decomposition by Heat or Strong Acid</span> </div> </a> <ul id="toc-Decomposition_by_Heat_or_Strong_Acid-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Copper_chips" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Copper_chips"> <div class="vector-toc-text"> <span class="vector-toc-numb">13.2</span> <span>Copper chips</span> </div> </a> <ul id="toc-Copper_chips-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-The_brown_ring_test" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#The_brown_ring_test"> <div class="vector-toc-text"> <span class="vector-toc-numb">13.3</span> <span>The brown ring test</span> </div> </a> <ul id="toc-The_brown_ring_test-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Reduction_to_nitrites" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Reduction_to_nitrites"> <div class="vector-toc-text"> <span class="vector-toc-numb">13.4</span> <span>Reduction to nitrites</span> </div> </a> <ul id="toc-Reduction_to_nitrites-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Reduction_to_Ammonia" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Reduction_to_Ammonia"> <div class="vector-toc-text"> <span class="vector-toc-numb">13.5</span> <span>Reduction to Ammonia</span> </div> </a> <ul id="toc-Reduction_to_Ammonia-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Sulphates" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Sulphates"> <div class="vector-toc-text"> <span class="vector-toc-numb">14</span> <span>Sulphates</span> </div> </a> <button aria-controls="toc-Sulphates-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Sulphates subsection</span> </button> <ul id="toc-Sulphates-sublist" class="vector-toc-list"> <li id="toc-Barium_Chloride" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Barium_Chloride"> <div class="vector-toc-text"> <span class="vector-toc-numb">14.1</span> <span>Barium Chloride</span> </div> </a> <ul id="toc-Barium_Chloride-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Lead_Nitrate/Lead_Acetate" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Lead_Nitrate/Lead_Acetate"> <div class="vector-toc-text"> <span class="vector-toc-numb">14.2</span> <span>Lead Nitrate/Lead Acetate</span> </div> </a> <ul id="toc-Lead_Nitrate/Lead_Acetate-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Manganate_Ion" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Manganate_Ion"> <div class="vector-toc-text"> <span class="vector-toc-numb">15</span> <span>Manganate Ion</span> </div> </a> <button aria-controls="toc-Manganate_Ion-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Manganate Ion subsection</span> </button> <ul id="toc-Manganate_Ion-sublist" class="vector-toc-list"> <li id="toc-H2S_test" class="vector-toc-list-item vector-toc-level-2"> 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id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><p><br /> </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Sulphides">Sulphides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=1" title="Edit section: Sulphides" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=1" title="Edit section's source code: Sulphides"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Sodium_Nitroprusside">Sodium Nitroprusside</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=2" title="Edit section: Sodium Nitroprusside" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=2" title="Edit section's source code: Sodium Nitroprusside"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Chemistry_Lab_Practical_for_students_of_class_XII.pdf" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Chemistry_Lab_Practical_for_students_of_class_XII.pdf/page1-220px-Chemistry_Lab_Practical_for_students_of_class_XII.pdf.jpg" decoding="async" width="220" height="285" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Chemistry_Lab_Practical_for_students_of_class_XII.pdf/page1-330px-Chemistry_Lab_Practical_for_students_of_class_XII.pdf.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Chemistry_Lab_Practical_for_students_of_class_XII.pdf/page1-440px-Chemistry_Lab_Practical_for_students_of_class_XII.pdf.jpg 2x" data-file-width="1275" data-file-height="1650" /></a><figcaption>test for anions</figcaption></figure> <p>Use <a href="https://en.wikipedia.org/wiki/Sodium_Nitroprusside" class="extiw" title="w:Sodium Nitroprusside">sodium nitroprusside</a>. In the presence of <a href="https://en.wikipedia.org/wiki/sulphide" class="extiw" title="w:sulphide">sulphide</a> ions a deep violet coloration is formed. [Fe(CN)<sub>5</sub>NO]<sup>4-</sup> complex anion formed in the presence of sulphide ions is the cause for this coloration, colouration is important. </p> <div class="mw-heading mw-heading3"><h3 id="Silver_Nitrate">Silver Nitrate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=3" title="Edit section: Silver Nitrate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=3" title="Edit section's source code: Silver Nitrate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>If a sulfide solution is reacted with silver nitrate, it forms a black precipitate of Ag<sub>2</sub>S. </p> <div class="mw-heading mw-heading3"><h3 id="Lead_Ethanoate">Lead Ethanoate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=4" title="Edit section: Lead Ethanoate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=4" title="Edit section's source code: Lead Ethanoate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>If the substance is soluble use <a href="https://en.wikipedia.org/wiki/lead_ethanoate" class="extiw" title="w:lead ethanoate">lead acetate</a> solution, if solid add dilute <a href="https://en.wikipedia.org/wiki/hydrochloric_acid" class="extiw" title="w:hydrochloric acid">hydrochloric acid</a> and test the gas with lead ethanoate paper. It is prepared by dipping a filter paper for some time in Lead acetate solution.If the salt in question is a sulphide an acrid smell of rotten eggs will be observed and the lead ethanoate will turn black, due to formation of solid black Lead sulfide powder. (CH<sub>3</sub>COO)<sub>2</sub>Pb + H<sub>2</sub>S -> PbS + 2(CH<sub>3</sub>COOH) </p> <div class="mw-heading mw-heading3"><h3 id="H2S">H<sub>2</sub>S</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=5" title="Edit section: H2S" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=5" title="Edit section's source code: H2S"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><b>The following two points do not fall in place here, kindly arrange them wherever they are best fit:</b> </p> <ul><li>When H2S is bubbled through a solution of Sodium sulphite or Sodium bisulphite, a white turbidity of sulfur is seen. What happens is, the S atom in sulphite/bisulphite (Oxidation state +4) and in H2S (Oxidation state -2) have coproportionated to give molecular sulfur in zero oxidation state. The reaction can be viewed as the reverse of a disproportionation reaction.</li></ul> <ul><li>When H2S is bubbled through acidified KMnO4 solution, it decolorises and a white turbidity is observed. This is because, the powerful oxidizing agent permanganate ion has oxidized the sulfide ion (-2) to zero oxidation state. In doing so, the permanganate ions themselves reduce to Mn<sup>2+</sup> ions, thus the purple/violet/pink color of the solution is diluted and eventually fades away as the manganous ions do not impart any color to the solution.</li></ul> <div class="mw-heading mw-heading2"><h2 id="The_nitrite_ion">The nitrite ion</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=6" title="Edit section: The nitrite ion" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=6" title="Edit section's source code: The nitrite ion"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The nitrite ion gives several reactions based on its redox properties. </p> <div class="mw-heading mw-heading3"><h3 id="I3-">I<sub>3</sub>-</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=7" title="Edit section: I3-" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=7" title="Edit section's source code: I3-"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When it reacts with the I<sub>3</sub>- anion, the nitrite ion reduces itself to nitric oxide. The student should check the oxidation states of nitrogen in both the cases. </p><p>NO<sub>2</sub><sup>-</sup> + 2I<sub>3</sub><sup>-</sup> + 2H<sup>+</sup> --> NO(g) + 3I<sub>2</sub>(aq) + H<sub>2</sub>O(l) </p><p>The yellow color of the I<sub>3</sub>- ions changes to a greenish tinge which later turns violet. This observation is made in the presence of an oxidising agent which oxidizes iodine from -⅓ to 0. The O.A. in our case is of course, the nitrite ion. </p><p>Before turning violet, a greenish tinge is observed because the increasing concentration of violet color and the decreasing concentration of yellow color during the reaction impart a greenish color. </p> <div class="mw-heading mw-heading3"><h3 id="Lead/Silver_Nitrates"><span id="Lead.2FSilver_Nitrates"></span>Lead/Silver Nitrates</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=8" title="Edit section: Lead/Silver Nitrates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=8" title="Edit section's source code: Lead/Silver Nitrates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Most lead and silver compounds show much the same characteristics in analysis. However, lead nitrite is soluble while silver nitrite is an insoluble white solid. </p><p>Therefore, to test for the presence of nitrite ions we can use silver and lead nitrate. No precipitate will be observed with lead nitrate, but a white precipitate will form when silver nitrate is added. </p><p>2NO<sub>2</sub><sup>-</sup> + Pb<sup>2+</sup> -> Pb(NO<sub>2</sub>)<sub>2</sub>(aq) </p><p>NO<sub>2</sub><sup>-</sup> + Ag<sup>+</sup> -> AgNO<sub>2</sub>(s) </p> <div class="mw-heading mw-heading2"><h2 id="The_cyanide_ions">The cyanide ions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=9" title="Edit section: The cyanide ions" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=9" title="Edit section's source code: The cyanide ions"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Ferric_ions">Ferric ions</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=10" title="Edit section: Ferric ions" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=10" title="Edit section's source code: Ferric ions"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When ferric ions are added to a solution of cyanide ions, no specific change in color is observed. However, if we add the ferric ions to the solution after adding thiosulphate or S<sub>2</sub><sup>2-</sup>, we get a blood red coloration of ferric thiocyanate. </p><p>Ferric thiocyanate is Fe(SCN)<sub>3</sub>. </p><p>Actually, this is a characteristic test for the presence of ferric ions and for thiocyanate ions. Cyanide ions are nowhere directly involved in the formation of ferric(III) thiocyanate. If we review the test procedure for the detection of cyanide ions, we find that we add, according to our choice, either thiosulphate ions or S<sub>2</sub><sup>2-</sup> ions. These ions disproportionate in the presence of cyanide ions, forming thiocyanate ions. It is these thiocyanate ions that eventually react with the added ferric ions to give the blood red complex formation </p><p>CN<sup>-</sup> + S<sub>2</sub>O<sub>3</sub><sup>2-</sup> -> SCN<sup>-</sup> + SO<sub>3</sub><sup>2-</sup> </p><p>CN<sup>-</sup> + S<sub>2</sub><sup>2-</sup> -> SCN<sup>-</sup> + S<sup>2-</sup> </p><p>Fe<sup>3+</sup> + SCN<sup>-</sup> -> Fe(SCN)<sup>2+</sup> </p> <div class="mw-heading mw-heading3"><h3 id="Metallic_copper">Metallic copper</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=11" title="Edit section: Metallic copper" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=11" title="Edit section's source code: Metallic copper"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>It is a popular fact that most metals react with either water or dilute acid solution to liberate hydrogen. This is a redox reaction in which the metal acts as a reducing agent, reducing the proton or hydrogen in water to hydrogen gas, oxidizing itself to a metal cation. </p><p>A classic example of this type of redox reaction is the reaction of metallic sodium with water. The reaction takes place and liberates enough heat to melt the sodium which then floats on a cushion of hydrogen gas. e.g., 2Na + 2H<sub>2</sub>O -> H<sub>2</sub> + 2NaOH. In terms of the ions involved in the reaction Na -> Na<sup>1+</sup> + e<sup>1-</sup> and then 2H<sup>1+</sup> + 2e<sup>1-</sup> -> H<sub>2</sub>. The same reaction occurs with any of the alkali metals in exactly the same way. </p><p>However, there are some metals like copper which will not react with either water or dilute acids in the same way. Quantitatively, Standard Electrode Potential is lower than that of hydrogen ions, meaning that more energy is required to form copper ions than the hydrogen ions can provide. [Note to editors --> Is this any better?] </p><p>However, if we add metallic copper to a solution containing cyanide ions, copper gives into the greed of forming that ultrastable cyano complex of itself. That is, equilibrium favours the formation of tetracyanocomplexcuprate(I) ions. This is the point - in presence of cyanide ions, copper oxidizes itself to form the +1 metal complex. But then, if an oxidation has occurred so must have a reduction. What is the reduction reaction? The formation of hydrogen (editors - formation from what? proton or water molecule?) is the involved reduction. </p><p><b>We conclude that an aqueous solution of KCN dissolves metallic copper, generally administered as copper turnings through, the formation of tetracyanocuprate(I) ions.</b> </p><p>(Note to editors --> Explain this anamlolous behaviour of copper through the quantitative aspects of electrochemistry and chemical equilibrium, short enough to maintain interest.) </p> <div class="mw-heading mw-heading4"><h4 id="Note_on_the_tetracyano_complex_of_copper">Note on the tetracyano complex of copper</h4><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=12" title="Edit section: Note on the tetracyano complex of copper" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=12" title="Edit section's source code: Note on the tetracyano complex of copper"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When H<sub>2</sub>S is bubbled through the cyano complex of ferrous/ferric/cuprous/cupric ions, no sulphide is precipitated. While with most other metal cations, metal sulphide does get precipitated. </p><p>e.g. tetracyanocadmiumate ions give CdS with H<sub>2</sub>S and dicyanoargentate (silver complex) give Ag<sub>2</sub>S. </p><p>This can be explained on the basis of equilibrium constants - solubility products and formation constants of the concerned sulphides and cyanocomplexes. (note to editors --> plz explain in a little more detail) </p> <div class="mw-heading mw-heading2"><h2 id="The_hypochlorite_ion">The hypochlorite ion</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=13" title="Edit section: The hypochlorite ion" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=13" title="Edit section's source code: The hypochlorite ion"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Adding a solution containing lead ions, such as lead nitrate, to a hypochlorite solution produces a brown precipitate of lead(IV) oxide. </p><p>2ClO<sup>-</sup> (aq) + Pb<sup>2+</sup> (aq) → PbO<sub>2</sub> (s) + 2Cl<sup>-</sup> (aq) </p><p>Adding hydrogen peroxide to sodium hypochlorite produces sodium chloride, water and oxygen. </p><p>ClO<sup>-</sup> (aq) + H<sub>2</sub>O<sub>2</sub> (l) → O<sub>2</sub> (g) + H<sub>2</sub>O (l) + Cl<sup>-</sup> (aq) </p> <div class="mw-heading mw-heading2"><h2 id="The_azide_ion">The azide ion</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=14" title="Edit section: The azide ion" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=14" title="Edit section's source code: The azide ion"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>On adding triiodide ions, the azide ion oxidizes to nitrogen and decolorisation is observed. . Triiodide ions are reduced to iodide ions, and nitrogen is produced. The colour of solution changes from yellow to colourless and a brisk effervescence is noted. </p><p>2N<sub>3</sub><sup>-</sup> -> 3N<sub>2</sub> + 2e<sup>-</sup> </p><p>I<sub>3</sub><sup>-</sup> + 3e<sup>-</sup> -> 3I<sup>-</sup> </p> <div class="mw-heading mw-heading2"><h2 id="The_acetate_ion">The acetate ion</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=15" title="Edit section: The acetate ion" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=15" title="Edit section's source code: The acetate ion"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Acidification">Acidification</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=16" title="Edit section: Acidification" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=16" title="Edit section's source code: Acidification"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Adding strong acid (such as HCl) to a concentrated acetate solution produces acetic acid, which emits a strong smell of vinegar. However, even if acetate is present, the vinegar smell may not be noticeable if the acetate is too dilute. </p> <div class="mw-heading mw-heading3"><h3 id="Esterification">Esterification</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=17" title="Edit section: Esterification" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=17" title="Edit section's source code: Esterification"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When a drop of concentrated sulphuric acid and ethanol are added, the distinctive smell of an ester can be observed. This applies to all carboxylic acids but is particularly useful in this case because the two reactants, acetic acid and ethanol, have distinctive smells which are replaced completely by different smell of the ester; in this case, ethyl acetate, which smells not unlike glue or nail polish remover. </p><p>CH<sub>3</sub>COOH + CH<sub>3</sub>CH<sub>2</sub>OH -> CH<sub>3</sub>COOCH<sub>2</sub>CH<sub>3</sub> + H<sub>2</sub>O </p><p>(The sulphuric acid is not shown as it is merely a catalyst, specifically a dehydrating agent.) </p> <div class="mw-heading mw-heading3"><h3 id="Ferric_Chloride">Ferric Chloride</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=18" title="Edit section: Ferric Chloride" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=18" title="Edit section's source code: Ferric Chloride"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When added to neutral FeCl<sub>3</sub> acetates produce a red coloration. </p><p>FeCl<sub>3</sub> + 3CH<sub>3</sub>COOH -> (CH<sub>3</sub>COO)<sub>3</sub>Fe + 3HCl </p><p>Neutral FeCl<sub>3</sub> is prepared by taking about an mL of FeCl<sub>3</sub> in a test tube and adding about few drops of dil. Na<sub>OH</sub> to give a permanent reddish brown precipitate.Ferric chloride is added to the test tube till the precipitate has JUST dissolved. The resultant solution is added to the salt solution containing acetate to give a red colouration. The acetate ion is confirmed by adding water to this mixture and warming till formation of red precipitate.A-LEVEL EXPERIMENT. </p> <div class="mw-heading mw-heading2"><h2 id="Thiosulphates">Thiosulphates</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=19" title="Edit section: Thiosulphates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=19" title="Edit section's source code: Thiosulphates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Thiosulphates are reducing agents. They can reduce I<sub>3</sub><sup>-</sup> ions to iodide ions which are colorless. However, it should be noted that this is not a confirmatory test as any reducing agent can do this. </p><p>2S<sub>2</sub>O<sub>3</sub><sup>2-</sup> -> S<sub>4</sub>O<sub>6</sub><sup>2-</sup> + 2e </p><p>I<sub>3</sub><sup>-</sup> +2e -> 3I<sup>-</sup> </p> <div class="mw-heading mw-heading3"><h3 id="Hydronium_ions">Hydronium ions</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=20" title="Edit section: Hydronium ions" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=20" title="Edit section's source code: Hydronium ions"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Adding dilute acid to a solution with thiosulphate ions yields a solution with precipitate, elemental sulfur, and release a burnt rubber smell (gaseous sulphur dioxide) </p><p>2H<sup>+</sup> + S<sub>2</sub>O<sub>3</sub><sup>2-</sup> -> S<sub>(s)</sub> + SO<sub>2(g)</sub> + H<sub>2</sub>O<sub>(l)</sub> </p> <div class="mw-heading mw-heading3"><h3 id="Ferric_ions_2">Ferric ions</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=21" title="Edit section: Ferric ions" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=21" title="Edit section's source code: Ferric ions"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>It also produces a momentary violet coloration with ferric ions. --->Expand<-- </p> <div class="mw-heading mw-heading3"><h3 id="Copper_Sulphate">Copper Sulphate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=22" title="Edit section: Copper Sulphate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=22" title="Edit section's source code: Copper Sulphate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>With copper sulphate, a white ppt. is obtained which dissolves in excess of thiosulphate to produce a colorless solution through the formation of a stable complex. </p><p>CuSO<sub>4</sub> + Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub> -> CuS<sub>2</sub>O<sub>3</sub> + Na<sub>2</sub>SO<sub>4</sub> </p><p>This test has to be carried out in such a way that initially the concentration of thiosulphate is low which then gradually increases enough to form the complex. The solution containing thiosulphate should be poured into the copper sulphate to prevent the changes being missed. </p> <div class="mw-heading mw-heading3"><h3 id="Silver_Nitrate_2">Silver Nitrate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=23" title="Edit section: Silver Nitrate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=23" title="Edit section's source code: Silver Nitrate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>This is a very peculiar reaction, because on the surface it seems as if the precipitate obtained is changing colors! </p><p>What actually happens is that when we add silver nitrate, a white ppt of silver thiosulphate is formed. This silver thiosulphate disproportionates to give silver sulphide and sulphuric acid, wherein as we know, silver sulphide is black. That is, on adding silver nitrate a white precipitate is obtained which changes to brown and finally to black. </p><p>S<sub>2</sub>O<sub>3</sub><sup>2-</sup> + 2AgNO<sub>3</sub> -> 2NO<sub>3</sub><sup>-</sup> + Ag<sub>2</sub>S<sub>2</sub>O<sub>3</sub> </p><p>Ag<sub>2</sub>S<sub>2</sub>O<sub>3</sub>(s) + H<sub>2</sub>O(l) -> H<sub>2</sub>SO<sub>4</sub>(aq) + Ag<sub>2</sub>S </p><p>Furthermore, in the presence of excess of thiosulphate ions the white ppt of Silver thiosulphate dissolves giving a colorless complex. </p> <div class="mw-heading mw-heading2"><h2 id="Thiocyanate_ions">Thiocyanate ions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=24" title="Edit section: Thiocyanate ions" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=24" title="Edit section's source code: Thiocyanate ions"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>SCN<sup>-</sup> ions have been discussed once in the testing of cyanide ions. </p><p>In fact, one of the characteristic tests for thiocyanate ions is the same reaction that we discussed over there. </p> <div class="mw-heading mw-heading3"><h3 id="Ferricthiocyanate">Ferricthiocyanate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=25" title="Edit section: Ferricthiocyanate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=25" title="Edit section's source code: Ferricthiocyanate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>With ferric ions, thiocyanate ions give a blood red coloration of Fe(SCN)<sub>3</sub>. This test is NOT given by ferrous ions - and hence is confirmatory for the presence of both ferric ions and for thiocyanate ions. </p><p>-->Check lingo<-- </p> <div class="mw-heading mw-heading3"><h3 id="Vogel's_test"><span id="Vogel.27s_test"></span>Vogel's test</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=26" title="Edit section: Vogel's test" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=26" title="Edit section's source code: Vogel's test"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>If Co<sup>2+</sup> ions are added to the thiocyanate ions a blue solution of tettrathiocyanatocobaltate is obtained. This complex on addition mercuric ions gives a Blue crystalline precipitate. </p><p>This ppt is NOT Mercuric tetrathiocyanatocobaltate! It is interesting to note that the actual precipitate is an isomer of the expected ppt - it is Cobalt(II) Tetrathiocyanatomercurate(II), that is the metal cations have switched places. </p><p><span style="color:red;"><b>If no effervescence is obtained with dilute HCl, heat the salt with Conc. H<sub>2</sub>SO<sub>4</sub></b></span> </p><p><span style="color:red;"><b>The following ions belong to this list:</b></span> </p> <div class="mw-heading mw-heading2"><h2 id="Fluorides">Fluorides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=27" title="Edit section: Fluorides" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=27" title="Edit section's source code: Fluorides"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Evolution_of_HF">Evolution of HF</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=28" title="Edit section: Evolution of HF" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=28" title="Edit section's source code: Evolution of HF"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When we add concentrated sulphuric acid to fluoride ions, they are protonated to give hydrogen fluoride. This is because hydrogen fluoride is a weak acid, its anion F<sup>-</sup> can be protonated back to the gas. </p><p>F<sup>-</sup> + H<sub>2</sub>SO<sub>4</sub> -> HF + HSO<sub>4</sub><sup>-</sup> </p><p>The extent to which hydrogen fluoride is produced is dependent on the initial concentration of the sulphuric acid. By Le Chatelier's equilibrium principle, a larger amount of the reactant H<sub>2</sub>SO<sub>4</sub>, coming from an increase in concentration, would drive the reaction towards the production of more gaseous hydrogen fluoride. </p><p>The question is, how do we know that HF has evolved? When we hold a glass rod at the mouth of the testtube, a white waxy deposit is obtained on the glass rod. This is because of the reaction of HF with Silica. (Glass rod - is of course nearly all silica!). </p><p>HF(g) + SiO<sub>2</sub>(s) -> SiF<sub>4</sub>(g) + H<sub>2</sub>0(l) </p><p>The silicon fluoride gas is easily hydrolyzed by the water released, and we get hydrogen silicofluoride and hydrogen silicate - the mixture which is the white waxy deposit in question. </p><p>3SiF<sub>4</sub>(g) + 4H<sub>2</sub>0(l) -> 2H<sub>2</sub>(SiF<sub>6</sub>)(s) + H<sub>4</sub>SiO<sub>4</sub>(s) </p><p>Question: Is is possible to detect HF or F<sup>-</sup> using Ca(NO<sub>3</sub>)<sub>2</sub>? </p><p>2 F<sup>-</sup><sub> (aq)</sub> + Ca(NO<sub>3</sub>)<sub>2</sub><sub>(aq)</sub> -> CaF<sub>2 (s)</sub> + 2 NO<sub>3</sub><sup>-</sup><sub> (aq)</sub> </p> <div class="mw-heading mw-heading3"><h3 id="Oxidation_of_fluorides">Oxidation of fluorides</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=29" title="Edit section: Oxidation of fluorides" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=29" title="Edit section's source code: Oxidation of fluorides"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>In this particular test, We added conc. H2SO4. H2SO4 is an oxidizing agent. When it is added to a fluoride salt, does it oxidize to molecular fluorine? Let us think for a second. Yes, we accept that Conc. H2SO4 is a pretty strong oxidizing agent, but the question is, is it strong enough to oxidize fluoride ions? The product of oxidation of fluoride ions is molecular fluorine - something which is rarer than anything. Molecular fluorine reacts with almost anything. It causes mayhem wherever it goes. So our answer is no. H2SO4 just can't oxidize fluoride ions into molecular fluorine. </p><p>-->Note to editors: This is the purpose of the text - to acquaint the reader with the various facts of chemistry and making them realize their importance in the real life. While this point doesn't exactly point out the high reactivity of fluorine, half a dozen scattered discussions can do enough to hammer this point! </p><p>Possible insertions - the problems involved in the electrolytic extraction of fluorine.<-- </p> <div class="mw-heading mw-heading2"><h2 id="Chlorides">Chlorides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=30" title="Edit section: Chlorides" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=30" title="Edit section's source code: Chlorides"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Conc._H2SO4">Conc. H<sub>2</sub>SO<sub>4</sub></h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=31" title="Edit section: Conc. H2SO4" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=31" title="Edit section's source code: Conc. H2SO4"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When concentrated H<sub>2</sub>SO<sub>4</sub> is added, chloride salts evolve colorless HCl gas. </p><p>Now the presence of this HCl gas can be detected in two ways. The first is to hold an ammonium hydroxide test tube near the mouth of the original solution. The HCl gas, if evolved, will react with NH4OH to give dense white fumes of NH4Cl. </p><p>Otherwise, we can use MnO2. Manganese in +4 state will be reduced to +2, oxidizing the chlorine in HCl to molecular chlorine gas - Cl2. Pale green (pale because of low concentration) Chlorine gas confirms that HCl was evolved. Chlorine gas has a bleaching action and should not be inhaled. </p> <div class="mw-heading mw-heading3"><h3 id="The_Silver_Nitrate_test">The Silver Nitrate test</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=32" title="Edit section: The Silver Nitrate test" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=32" title="Edit section's source code: The Silver Nitrate test"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>AgCl is a precipitate. So, if a silver nitrate solution is added to a sample of the being tested solution, a white ppt. is obtained. This precipitated Agcl is soluble in an excess of Ammonium Hydroxide solution because of the formation of [Ag(NH3)2]<sup>+</sup> complex ions. </p><p>if we note carefully, the ammine complex is the same one that is used in the silver mirror test (Tollen's test) for the detection of aldehydes. The reaction, if we recall, was a redox reaction in which the silver (I) is reduced to metallic (0) silver mirror, and the aldehyde being oxidized to an ate ion. </p> <div class="mw-heading mw-heading3"><h3 id="The_Chromyl_Chloride_test">The Chromyl Chloride test</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=33" title="Edit section: The Chromyl Chloride test" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=33" title="Edit section's source code: The Chromyl Chloride test"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>It should be noted that this test is not for a solution containing the solvated ions. Chromyl chloride test is performed on the salt in solid state. </p><p>Solid salt is mixed with Solid Potassium Dichromate and Conc. H<sub>2</sub>SO<sub>4</sub>. If the salt is a chloride, on heating deep red vapors of Chromyl Chloride (CrO<sub>2</sub>Cl<sub>2</sub>) are evolved. </p><p>Some chemists still bear a doubt, because the deep red vapors bear some resemblance to NO<sub>2</sub> and Br<sub>2</sub> vapors. They can be distinguished, though. </p><p>If these Chromyl Chloride vapors are passed through a dilute NaOH solution, it turns yellow. Most of us might have already guessed that the color is due to the formation of the Chromate ions. Indeed, the guess is true. This is then how we resolve our doubts and say that the salt is a chloride. </p><p>It is not unwise to note here that most chromates are yellow in color, with the notable exceptions being Ag<sub>2</sub>CrO<sub>4</sub> and Hg<sub>2</sub>CrO<sub>4</sub>. Both are red! </p><p><b>Predominantly covalent chlorides like HgCl<sub>2</sub> and alkyl chlorides do not offer this test. </b> The real confirmation is adding acetic acid followed by lead acetate to the yellow solution which gives a pale yellow precipitate of lead chromate. </p> <div class="mw-heading mw-heading2"><h2 id="Bromides/Iodides"><span id="Bromides.2FIodides"></span>Bromides/Iodides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=34" title="Edit section: Bromides/Iodides" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=34" title="Edit section's source code: Bromides/Iodides"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Conc._H2SO4_2">Conc. H2SO4</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=35" title="Edit section: Conc. H2SO4" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=35" title="Edit section's source code: Conc. H2SO4"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>With conc. H2SO4, the florides/chlorides gave HF/HCl respectively. However, the bromides and iodides are oxidized to molecular bromine and iodine respectively! </p><p>So, in case of the reaction of iodides/bromides with Conc. H2SO4, bromides give deep brown vapors of Br2, while iodides give violet vapors of iodine. </p> <div class="mw-heading mw-heading3"><h3 id="Silver_nitrate_solution">Silver nitrate solution</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=36" title="Edit section: Silver nitrate solution" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=36" title="Edit section's source code: Silver nitrate solution"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>With silver nitrate solution, bromides give a pale yellow ppt. of AgBr which is partially soluble in NH4OH. Iodides give a yellow ppt of AgI which is insoluble in ammonium hydroxide. </p><p>-->Explain this point with reference to Solubility Product and formation constant of the concerned compounds. We need not give a numerical explanation! We just want to emphasize that Inorganic Chemistry is not plain mugging up. </p> <div class="mw-heading mw-heading3"><h3 id="The_Chloroform_test">The Chloroform test</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=37" title="Edit section: The Chloroform test" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=37" title="Edit section's source code: The Chloroform test"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Take the solution and add an equal amount of chloroform/CHCl3 to it. Add chlorine water and shake vigorously. Watch the change in color of the non-aqueous layer. </p><p>If iodide/bromide ions are present, they would be oxidized to Iodine/Bromine respectively. Iodine would impart a violet color to the non-aqueous layer while if bromine is created it will give out a reddish color to the non-aqueous layer. </p><p>The same reaction will also occur if dichloromethane is added in replacement of the chloroform. </p> <div class="mw-heading mw-heading2"><h2 id="Oxalate_ions">Oxalate ions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=38" title="Edit section: Oxalate ions" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=38" title="Edit section's source code: Oxalate ions"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The reactions for oxalate ions- 2MnO<sub>4</sub>- + 16H+ + 5C<sub>2</sub>O<sub>4</sub><sup>-2</sup> ---------> 2Mn<sup>+2</sup> +8H<sub>2</sub>O + 10 CO<sub>2</sub> Oxalate ions are C<sub>2</sub>O<sub>4</sub><sub>--</sub> </p> <div class="mw-heading mw-heading3"><h3 id="Conc._H2SO4_3">Conc. H<sub>2</sub>SO<sub>4</sub></h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=39" title="Edit section: Conc. H2SO4" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=39" title="Edit section's source code: Conc. H2SO4"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Concentrated sulphuric acid decomposes oxalate ions into carbon monoxide and carbon dioxide. Readers shouldn't take long to realize that the oxalate ions have decomposed through a disproportionation reaction. If the evolution of the two gases is confirmed, we can say that sulphuric acid reacted with oxalate ions. </p><p>If the evolved gaseous mixture is passed through limewater, it will turn milky and finally colourless. Carbon Monoxide in the mixture will burn with a blue flame to produce carbon dioxide. The two gases are confirmed in this way, confirming the presence of the oxalate ion. </p> <div class="mw-heading mw-heading3"><h3 id="Acidified_Potassium_Permanaganate_solution">Acidified Potassium Permanaganate solution</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=40" title="Edit section: Acidified Potassium Permanaganate solution" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=40" title="Edit section's source code: Acidified Potassium Permanaganate solution"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Acidified KMnO4 is an oxidizing agent. It will oxidize the oxalate ions into carbon dioxide. In the process, it will decolorize because of the reduction of the violet manganate ions into colorless manganous ions. </p><p>Now the question is, how do we know that the decolorization was due to oxalate ions? KMnO4 solution is decolorized each time the manganate ions oxidize ANYTHING. </p><p>The answer lies again, in the detection of the carbondioxide gas. Once the gas is confirmed, oxalate ions have been virtually confirmed. </p> <div class="mw-heading mw-heading3"><h3 id="Calcium_chloride_solution">Calcium chloride solution</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=41" title="Edit section: Calcium chloride solution" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=41" title="Edit section's source code: Calcium chloride solution"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Aqueous solution of oxalate ions give a white precipitate of calcium oxalate which is insoluble in acetic acid. </p> <div class="mw-heading mw-heading2"><h2 id="Nitrates">Nitrates</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=42" title="Edit section: Nitrates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=42" title="Edit section's source code: Nitrates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Decomposition_by_Heat_or_Strong_Acid">Decomposition by Heat or Strong Acid</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=43" title="Edit section: Decomposition by Heat or Strong Acid" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=43" title="Edit section's source code: Decomposition by Heat or Strong Acid"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>All nitrate salts are decomposed by heat or dilute sulphuric acid to produce reddish brown fumes of nitrogen dioxide. </p><p>2Cu(NO<sub>3</sub>)<sub>2</sub>(aq) -> 2CuO(aq) + 4NO<sub>2</sub>(g) + O<sub>2</sub>(g) </p> <div class="mw-heading mw-heading3"><h3 id="Copper_chips">Copper chips</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=44" title="Edit section: Copper chips" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=44" title="Edit section's source code: Copper chips"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>To the Aqueous solution of the salt when we added conc. sulphuric acid, and then copper chips are added, Dark brown solution forms. It forms due to acid of sulphur. </p> <div class="mw-heading mw-heading3"><h3 id="The_brown_ring_test">The brown ring test</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=45" title="Edit section: The brown ring test" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=45" title="Edit section's source code: The brown ring test"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When a freshly prepared acidified solution of ferrous sulphate is added to a solution of nitrate ions, in the presence of concentrated H<sub>2</sub>SO<sub>4</sub>, a deep brown ring is formed. </p><p>This deep brown ring is due to the formation of the complex sphere [Fe(H<sub>2</sub>O)<sub>5</sub>NO]<sup>2+</sup>. In this form, the Fe ion is in both its +1 and +2 oxidation states, and oscillates between the two. This means that even a slight disturbance in the medium will disturb the complex. It is for this reason that the acidified ferrous sulphate is added drop-wise and allowed to roll down the walls of the test tube, this minimises any disturbance that would destroy the ring. It reacts upon contact with the medium, and forms the mentioned complex, but only at the edges, forming the characteristic brown ring. </p><p>The oscillation occurs in the following two ways </p><p>i) The NO ion loses an electron to the Fe2+ ion forming Fe<sup>1+</sup> and NO<sup>1+</sup> NO -> NO<sup>1+</sup> + e<sup>1-</sup> Fe<sup>2+</sup> + e<sup>1-</sup> -> Fe<sup>1+</sup> </p><p>ii) The Fe<sup>1+</sup> returns the electron to the NO<sup>1+</sup> forming NO and Fe<sup>2+</sup> Fe<sup>1+</sup> -> Fe<sup>2+</sup> + e<sup>1-</sup> NO<sup>1+</sup> + e<sup>1-</sup> -> NO </p><p>It is worth noting that it is very rare to find iron in its (I) oxidation state, (II) and (III) are much more common </p> <div class="mw-heading mw-heading3"><h3 id="Reduction_to_nitrites">Reduction to nitrites</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=46" title="Edit section: Reduction to nitrites" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=46" title="Edit section's source code: Reduction to nitrites"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Reduction_to_Ammonia">Reduction to Ammonia</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=47" title="Edit section: Reduction to Ammonia" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=47" title="Edit section's source code: Reduction to Ammonia"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The NItrate ion can easily be reduced to ammonia with either Devardas Alloy or Aluminium Foil. The aluminium is a very powerful reducing agent, and this combined with heating causes the nitrate ions to form ammonia gas. This can be tested for by holding a piece of damp red litmus paper over the end of the test tube. The ammonia will form alkaline ammonium ions in the water and turn the paper blue. </p><p>4NO<sub>3</sub><sup>-</sup>(aq) + 6H<sub>2</sub>0(l) -> 4NH<sub>3</sub>(g) + 9O<sub>2</sub>(g) </p><p>Aluminium powder is not shown as it merely catalyses the reaction. </p> <div class="mw-heading mw-heading2"><h2 id="Sulphates">Sulphates</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=48" title="Edit section: Sulphates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=48" title="Edit section's source code: Sulphates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Barium_Chloride">Barium Chloride</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=49" title="Edit section: Barium Chloride" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=49" title="Edit section's source code: Barium Chloride"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The addition of a sulphate to a barium chloride solution produces a white precipitate of barium sulphate. This precipitate is very insoluble, not dissolving in any common laboratory reagents. </p><p>Magnesium Sulphate + Barium Chloride -> Barium Sulphate + Magnesium Chloride </p><p>MgSO<sub>4</sub>(aq) + BaCl<sub>2</sub>(aq) -> BaSO<sub>4</sub>(s) + MgCl<sub>2</sub>(aq) </p> <div class="mw-heading mw-heading3"><h3 id="Lead_Nitrate/Lead_Acetate"><span id="Lead_Nitrate.2FLead_Acetate"></span>Lead Nitrate/Lead Acetate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=50" title="Edit section: Lead Nitrate/Lead Acetate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=50" title="Edit section's source code: Lead Nitrate/Lead Acetate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>A similar reaction to the above, a white precipitate of lead sulphate is formed. Again this is very difficult to dissolve in common reagent like water, but dissolves in Sodium hydroxide and to a much extent in Ammonium acetate solution. </p><p>PbNO<sub>3</sub>(aq) + MgSO<sub>4</sub>(aq) -> PbSO<sub>4</sub>(s) + MgNO<sub>3</sub>(aq) </p><p>(CH<sub>3</sub>COO)<sub>2</sub>Pb(aq) + K<sub>2</sub>SO<sub>4</sub>(aq) -> PbSO<sub>4</sub>(s) + 2CH<sub>3</sub>COOK(aq) </p> <div class="mw-heading mw-heading2"><h2 id="Manganate_Ion">Manganate Ion</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=51" title="Edit section: Manganate Ion" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=51" title="Edit section's source code: Manganate Ion"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="H2S_test">H<sub>2</sub>S test</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=52" title="Edit section: H2S test" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=52" title="Edit section's source code: H2S test"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The oxidising properties of potassium manganate allow it to oxidise hydrogen sulphide rapidly from oxidation state (II) to 0, reducing itself to manganese ions. These do not impart any colour to the solution, yet the sulphur precipitate forms a white cloud as the purple colouration of manganate ions disappears. </p><p>2S<sup>2-</sup> -> S<sub>2</sub> + 4e </p><p>MnO<sub>4</sub><sup>2-</sup> + 4e<sup>-</sup> -> Mn<sup>2+</sup> + 2O<sub>2</sub> </p> <div class="mw-heading mw-heading2"><h2 id="Borates">Borates</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=53" title="Edit section: Borates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=53" title="Edit section's source code: Borates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Ethyl_Alcohol">Ethyl Alcohol</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=54" title="Edit section: Ethyl Alcohol" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=54" title="Edit section's source code: Ethyl Alcohol"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>on adding ethyl alcohol we get ethyl borate on expose to flame it gives greenish yellow colour flame. </p> <div class="mw-heading mw-heading2"><h2 id="Ortho-Phosphates">Ortho-Phosphates</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=55" title="Edit section: Ortho-Phosphates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=55" title="Edit section's source code: Ortho-Phosphates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Ammonium_Molybdate">Ammonium Molybdate</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=56" title="Edit section: Ammonium Molybdate" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=56" title="Edit section's source code: Ammonium Molybdate"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>When added to phosphate ions, warmed with nitric acid, forms a canary yellow precipitate of ammonium phosphorous molybdate.The same yellow canary colour is also given by arsenic salts after treating with Nitric acid. Confirmatory test for presence of phosphates.<br /> PO<sub>4<sup>3-</sup></sub> + 12(NH<sub>4</sub>)<sub>2</sub>MoO<sub>4</sub> + 21HNO<sub>3</sub> + 3H<sup>+</sup> -> (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub>·12MoO<sub>3</sub>↓ + 21NH<sub>4</sub>NO<sub>3</sub> + 12H<sub>2</sub>O </p> <div class="mw-heading mw-heading2"><h2 id="Carbonates_and_Bicarbonates">Carbonates and Bicarbonates</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&veaction=edit&section=57" title="Edit section: Carbonates and Bicarbonates" class="mw-editsection-visualeditor"><span>edit</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&action=edit&section=57" title="Edit section's source code: Carbonates and Bicarbonates"><span>edit source</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>In the presence of carbonate (CO<sub>3</sub><sup>2-</sup>) or bicarbonate (HCO<sub>3</sub><sup>-</sup>) ion, the addition of concentrated strong acid (e.g. HCl) causes the evolution of CO<sub>2</sub> gas, resulting in fizzing or bubbling. To determine which is present, MgSO<sub>4</sub> is added to the salt solution. A white precipitate at low temperatures indicates carbonate while precipitation upon heating confirms bicarbonate. </p></div><noscript><img src="https://login.wikimedia.org/wiki/Special:CentralAutoLogin/start?type=1x1" alt="" width="1" height="1" style="border: none; position: absolute;"></noscript> <div class="printfooter" data-nosnippet="">Retrieved from "<a dir="ltr" href="https://en.wikibooks.org/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&oldid=4368407">https://en.wikibooks.org/w/index.php?title=Inorganic_Chemistry/Qualitative_Analysis/Tests_for_anions&oldid=4368407</a>"</div></div> <div id="catlinks" class="catlinks" data-mw="interface"><div id="mw-normal-catlinks" class="mw-normal-catlinks"><a href="/wiki/Special:Categories" title="Special:Categories">Category</a>: <ul><li><a href="/wiki/Category:Book:Inorganic_Chemistry" title="Category:Book:Inorganic Chemistry">Book:Inorganic Chemistry</a></li></ul></div></div> </div> </main> </div> <div class="mw-footer-container"> <footer id="footer" class="mw-footer" > <ul id="footer-info"> <li id="footer-info-lastmod"> This page was last edited on 5 February 2024, at 00:48.</li> <li id="footer-info-copyright">Text is available under the <a rel="nofollow" class="external text" href="//creativecommons.org/licenses/by-sa/4.0/">Creative Commons Attribution-ShareAlike License</a>; additional terms may apply. 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