- 1(current)
Q. No.Given below are two statements:
| Assertion (A): | An aqueous solution of ammonium carbonate is basic. |
| Reason (R): |
The acidic or basic nature of a salt solution of a salt of a weak acid and a weak base depends on the Ka and Kb values of the acid and the base forming it. |
| 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. | (A) is false but (R) is true. |
The pH of neutral water at is 7.0. As the temperature increases, ionisation of water increases. However, the concentration of H+ ions and OH- ions is equal. The pH of pure water at is:
| 1. | Equal to 7.0 | 2. | Greater than 7.0 |
| 3. | Less than 7.0 | 4. | Equal to zero |
The ionisation constant of an acid, Ka , is the measure of the strength of an acid. The Ka values of acetic acid, hypochlorous acid and formic acid are and , respectively. The correct order of pH value of 0.1 mol dm-3 solutions of these acids is -
1. Acetic acid > hypochlorous acid > formic acid
2. Hypochlorous acid < acetic acid > formic acid
3. Formic acid > hypochlorous acid > acetic acid
4. Formic acid < acetic acid < hypochlorous acid
The value of the pH of \(0.01 \) \(\text{mol dm}^{-3} \)\(\text{CH}_3\text{COOH}\) \(\left(K_a=1.74 \times 10^{-5}\right)\) is:
| 1. | 3.4 | 2. | 3.6 |
| 3. | 3.9 | 4. | 3.0 |
- 1(current)
Q. No.
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