Q. No.1. \(3.022 \times 10^{-16}\)
2. \(3.022 \times 10^{13} ~\)
3. \(6.022 \times 10^{7} ~\)
4. \(6.022 \times 10^{23} ~\)
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. What will be the pH of pure water at 60°C ?
| 1. | Equal to 7.0 | 2. | Greater than 7.0 |
| 3. | Less than 7.0 | 4. | Equal to zero |
(log 55 = 1.74)
| 1. | 7.00 | 2. | 7.87 |
| 3. | 5.13 | 4. | 6.13 |
The concentration of hydrogen ion in a sample of soft drink is . The pH of the soft drink will be:
| 1. | 3.14
|
2. | 2.42
|
| 3. | 11.58
|
4. | 6.00 |
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. | 3 | 2. | 2 |
| 3. | 4 | 4. | 1 |
The ionization constant of HF is 3.2 × 10–4 and its solution concentration is 0.02 M. The pH of the solution is:
1. 3.45
2. 2.62
3. 4.21
4. 1.89
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. |
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