Revision Notes for Class 10 Chemistry: Qualitative Analysis of Salts
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Review Qualitative Analysis of Salts for Class 10 Chemistry
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Group Reactions of the Metal Ions
| Group | Group reagent | Precipitates and tests |
|---|---|---|
| Silver group: Ag\( ^+ \), Hg\( _2 \)\( ^{2+} \), Pb\( ^{2+} \) | Dilute HCl | White AgCl, Hg\( _2 \)Cl\( _2 \), PbCl\( _2 \). PbCl\( _2 \) dissolves in hot water; AgCl turns violet in light and dissolves in NH\( _4 \)OH; Hg\( _2 \)Cl\( _2 \) turns black with NH\( _4 \)OH. Lead gives yellow PbI\( _2 \) with KI that dissolves in hot water and returns as golden spangles. |
| Copper group: Hg\( ^{2+} \), Pb\( ^{2+} \), Cu\( ^{2+} \) | H\( _2 \)S with dilute HCl | Black HgS, PbS, CuS. Copper: pale blue precipitate with NH\( _4 \)OH, dissolving in excess to a deep blue solution. Mercuric: scarlet HgI\( _2 \) with KI, dissolving in excess. |
| Iron group: Fe\( ^{2+} \), Fe\( ^{3+} \), Al\( ^{3+} \) | NH\( _4 \)Cl then NH\( _4 \)OH | Reddish-brown Fe(OH)\( _3 \), white Al(OH)\( _3 \) (dissolves in excess NaOH). Ferric: blood-red with thiocyanate and Prussian blue with ferrocyanide. Ferrous: Turnbull's blue with ferricyanide. |
| Zinc group: Zn\( ^{2+} \), Mn\( ^{2+} \) | H\( _2 \)S in NH\( _4 \)Cl and NH\( _4 \)OH | White ZnS, flesh-coloured MnS. Zn(OH)\( _2 \) dissolves in excess NaOH to give zincate. |
| Alkaline earth group: Ca\( ^{2+} \), Ba\( ^{2+} \) | (NH\( _4 \))\( _2 \)CO\( _3 \) with NH\( _4 \)Cl and NH\( _4 \)OH | White CaCO\( _3 \), BaCO\( _3 \). Flames: calcium brick red, barium apple green. Ba gives yellow BaCrO\( _4 \) with K\( _2 \)CrO\( _4 \) and white BaSO\( _4 \) even from dilute solution; Ca gives white calcium oxalate. |
| Alkali group: Mg\( ^{2+} \), Na\( ^+ \), K\( ^+ \), NH\( _4 \)\( ^+ \) | None; tested singly | Mg: white MgNH\( _4 \)PO\( _4 \) with Na\( _2 \)HPO\( _4 \) in ammoniacal solution. NH\( _4 \)\( ^+ \): ammonia on warming with NaOH (turns red litmus blue, white fumes with HCl, brown precipitate with Nessler's reagent). Sodium: golden-yellow flame. Potassium: lilac flame (crimson through blue glass). |
Why the reagents are chosen as they are: the acid in the copper-group test keeps the sulphide ion concentration low so that sulphides of zinc and manganese do not precipitate; NH\( _4 \)Cl before NH\( _4 \)OH lowers the hydroxide ion concentration, so that only the least soluble hydroxides (Fe and Al) form in the iron group.
Tests for Acid Radicals
| Radical | Test | Observation |
|---|---|---|
| Carbonate | Dilute HCl; pass gas into lime water | Effervescence of CO\( _2 \); lime water turns milky and clears again with excess gas |
| Sulphide | Dilute HCl; lead acetate paper | Rotten-egg gas H\( _2 \)S; paper turns black |
| Sulphite | Dilute HCl; acidified K\( _2 \)Cr\( _2 \)O\( _7 \) paper | SO\( _2 \), burning-sulphur smell; paper turns green |
| Chloride | Concentrated H\( _2 \)SO\( _4 \); then AgNO\( _3 \) | HCl fumes (white fumes with NH\( _3 \)); white AgCl soluble in dilute NH\( _4 \)OH |
| Bromide | Concentrated H\( _2 \)SO\( _4 \); AgNO\( _3 \); CS\( _2 \) and chlorine water | Brown bromine vapour; pale yellow AgBr; orange-red CS\( _2 \) layer |
| Iodide | Concentrated H\( _2 \)SO\( _4 \); Pb(NO\( _3 \))\( _2 \) | Violet iodine vapour; yellow PbI\( _2 \) |
| Nitrate | FeSO\( _4 \) and concentrated H\( _2 \)SO\( _4 \) poured down the side of the tube; heating | Brown ring at the junction; brown NO\( _2 \) fumes on heating lead nitrate |
| Sulphate | BaCl\( _2 \) solution | White BaSO\( _4 \), insoluble in dilute HCl |
| Phosphate | Nitric acid and ammonium molybdate, boiled | Yellow precipitate of ammonium phosphomolybdate |
Hard and Soft Water
1. Water that lathers freely with soap is soft; water that needs much soap before a permanent lather is hard.
2. Temporary hardness is due to calcium and magnesium bicarbonates. It is removed by boiling (the bicarbonates change to insoluble carbonates) or by Clark's process (adding the correct amount of slaked lime).
3. Permanent hardness is due to chlorides and sulphates of calcium and magnesium. Boiling does not remove it. It is removed by washing soda (sodium carbonate), which precipitates the carbonates, or by passing the water through permutit (sodium aluminium silicate).
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