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**Q. 1. 0.1 M NaOH is titrated with 0.1 M HA till the end point; K _{a} for HA is 5.6 × 10^{–6} and degree of hydrolysis is less compared to 1. Calculate pH of the resulting solution at the end point.**

**Ans. **9

**Solution. **HA + NaOH → NaA + H 2O

At the end point, the solution contains only NaA whose concentration is 0.1/2 = 0.05 M

Since the salt NaA is formed by strong alkali (NaOH) and weak acid HA (indicated by its low K_{a} value), its pH can be evaluated by the following relation.

**Q. 2. The dissociation constant of a substituted benzoic acid at 25°C is 1.0 × 10 ^{–4}. The pH of a 0.01 M solution of its sodium salt is**

**Ans. **8

**Solution. **pH of sodium salt of weak acid

**Q. 3. Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is **

**KCN, K _{2}SO_{4}, (NH_{4})_{2}C_{2}O_{4}, NaCl, Zn(NO_{3})_{2}, FeCl_{3}, K_{2}CO_{3}, NH_{4}NO_{3} and LiCN**

**Ans. **3

**Solution. **KCN, K_{2}CO_{3} and LiCN are the salts of weak acid and strong base. So, their aqueous solutions turns red litmus paper blue.

**Q. 4. The total number of diprotic acids among the following is: **

**H _{3}PO_{4}, H_{2}SO_{4}, H_{3}PO_{3}, H_{2}CO_{3}, H_{2}S_{2}O_{7}, H_{3}BO_{3}, H_{3}PO_{2}, H_{2}CrO_{4} and H_{2}SO_{3}.**

**Ans. **6

**Solution. **Diprotic acids are H_{2}SO_{4}, H_{3}PO_{3}, H_{2}CO_{3}, H_{2}S_{2}O_{7}, H_{2}CrO_{4} and H_{2}SO_{3}.

**Q. 5. In 1 L saturated solution of AgCl [Ksp(AgCl) = 1.6 x 10 ^{–10}], 0.1 mol of CuCl [K_{sp}(CuCl) = 1.0 x 10^{–6}] is added. The resultant concentration of Ag^{+} in the solution is 1.6 x 10^{–x}.**

**The value of “x” is**

**Ans. **7

**Solution. **Let the solubility of AgCl is x mol litre^{-1} and that of CuCl is y mol litre^{-1}

∴ K_{sp }of AgCl = [Ag^{+}] [Cl^{–}]

1.6 × 10^{–10} = x (x + y) ....(i)

Similarly, K_{sp} of CuCl = [Cu^{+}][Cl^{–}]

1.6 × 10^{–6} = y(x + y) … (ii)

On solving, (i) and (ii)

[Ag^{+}] = 1.6 × 10^{–7} ∴ x = 7

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