Give a chemical test to distinguish between the following:

(i) Sodium carbonate and sodium sulphate

(ii) Potassium chloride and potassium nitrate

(iii) Copper carbonate and copper sulphite

(iv) Lead chloride and lead sulphide

(v) Iron (II) sulphate and iron (III) sulphate

(vi) Calcium sulphate and zinc sulphate

(vii) Lead nitrate and zinc nitrate

(viii) Copper sulphate and calcium sulphate

(ix) Manganese dioxide and copper (II) oxide

(x) dil. HCl, dil. HNO₃, dil. H₂SO₄.

[explain the procedure for the preparation of the solutions for the above tests wherever required]

Identify the cation [positive ion] and anion [negative ion] in - A, B and C. Also identify P, Q, R, S, T, U, V, W.

(a) Substance 'A' is water soluble and gives a curdy white precipitate 'P' with silver nitrate solution. 'P' is soluble in ammonium hydroxide but insoluble in dil. HNO₃. Substance 'A' reacts with ammonium hydroxide solution to give a white precipitate 'Q' soluble in excess of NH₄OH.

(b) A solution of substance 'B' is added to barium chloride solution. A white ppt. 'R' is formed, insoluble in dil. HCl or HNO₃. A dirty green ppt. 'S' is formed on addition of ammonium hydroxide to a solution of 'B' and the precipitate is insoluble in excess of ammonium hydroxide.

(c) Substance 'C' is a coloured, crystalline salt which on heating decomposes leaving a black residue 'T'. On addition of copper turnings and conc. H₂SO₄ to 'C' a coloured acidic gas 'U' is evolved on heating. A solution of 'C' is added to NaOH soln. until in excess. A pale blue ppt. 'P' is obtained insoluble in excess of NaOH. A solution of 'C' is then added to NH₄OH soln. in excess to give an inky blue solution 'V'. A solution of 'C' is warmed and hydrogen sulphide gas is passed through it. A black ppt. 'W' appears.

Select the correct 'anion' of a salt from the anions given, which matches with description 1 to 5.

A: CO₃^2-, B: NO₃^1-, C: SO₄^2-, D: Cl^-, E: S^2-

1. The salt soln. reacts with AgNO₃ soln. to give a white ppt. insoluble in dil. HNO₃.
2. The salt soln. reacts with Ba(NO₃)₂ soln. to give a white ppt. insoluble in dil. HNO₃.
3. The salt soln. reacts with Ba(NO₃)₂ soln. to give a white ppt. soluble in dil. HNO₃ but insoluble in dil. H₂SO₄.
4. The salt reacts with dil. H₂SO₄ on heating evolving a gas which turns KMnO₄ soln. pink to colourless.
5. The salt reacts with conc. H₂SO₄ on heating evolving a coloured gas which turns potassium iodide paper brown.

Give balanced equations for the conversions A and B.

1. $\text{Metallic carbonate} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{Ba(NO}$3)2} \text{White precipitate} \quad \raisebox{0.35em}{B} \space \xrightarrow{\text{dil. HCl}} \text{precipitate dissolves}
2. $\text{Metallic sulphide} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{Pb(CH}$3{\text{COO}})2 \text{ soln.}} \text{black precipitate }
3. $\text{Metallic salt} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{BaCl}_2 \text{ soln.}} \text{Barium sulphite} \quad \raisebox{0.35em}{B} \space \xrightarrow{\text{dil. HCl}} \text{Barium chloride}$
4. $\text{Metallic chloride} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{conc. H}$2\text{SO}4\Delta} \text{Gas evolved} \quad \raisebox{0.35em}{B} \space \xrightarrow{\text{AgNO}_3} \text{White precipitate}
5. $\text{Metallic salt} \quad \raisebox{0.35em}{A} \space \xrightarrow{\text{BaCl}_2} \text{White precipitate insoluble in dil. HCl}$