Q. No.When 10 ml of 0.1 M acetic acid (pKa=5.0) is titrated against 10 ml of 0.1 M
ammonia solution (pKb=5.0),
the pH at equivalence point will be:
| 1. | 9.0 | 2. | 6.0 |
| 3. | 5.0 | 4. | 7.0 |
The salt solution that is basic in nature is:
1. Ammonium chloride.
2. Ammonium sulphate.
3. Ammonium nitrate.
4. Sodium acetate.
The degree of hydrolysis of the salt is independent of the concentration of a solution:
1. NH4CI
2. NH4CN
3. (NH4)2SO4
4. All of the above
| Assertion (A): | The aqueous solution of \(CH_3COONa\) is alkaline in nature. |
| Reason (R): | Sodium acetate undergoes cationic hydrolysis. |
| 1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |
| 3. | (A) is true but (R) is false. |
| 4. | Both (A) and (R) are false. |
The ionization constant of chloroacetic acid is 1.35 × 10–3. The pH of a 0.1 M acid solution will be:
| 1. | 1.94
|
2. | 6.14
|
| 3. | 3.23
|
4. | 5.64 |
The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 10%. If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be -
1. 5 %
2. 10 %
3. 20 %
4. None of the above
If the pH of 0.1 M NaCN solution is 11, then the percentage hydrolysis will be:
1. 0.1%
2. 1%
3. 0.01%
4. 10%
The ionization constant of nitrous acid is 4.5 × 10–4. The pH of a 0.04 M sodium nitrite solution will be:
| 1. | 2.56 | 2. | 6.14 |
| 3. | 7.96 | 4. | 11.74 |
A 0.02 M solution of pyridinium hydrochloride has a pH of 3.44. The ionization constant of pyridine will be:
| 1. | 2. | ||
| 3. | 4. |
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