The pH value of a 0.01 M solution of an organic acid is 4.15. The pKa of the acid will be:

$1.$ $8.95$
$2.$ $1.43$
$3.$ $3.56$
$4.$ $6.30$

Subtopic:  Ionisation Constant of Acid, Base & Salt |
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A 0.001 M aniline solution has a pH of:
($$K_b = 4.27 \times 10^{-10}$$)

 1 6.19 2 7.81 3 8.34 4 9.81
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The degree of ionization of 0.05 M acetic acid is:

(pKa = 4.74)

 1 2 3 4
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The percentage ionization of 0.02 M dimethylamine solution if it also contains 0.1 M NaOH solution (Kb of dimethylamine = 5.4 × 10–4) will be:

 1 0.54% 2 0.05% 3 5.40% 4 54.00%

Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The pH of a 0.1 M solution of cyanic acid (HCNO) is 2.34. The ionization constant of the acid will be:

$1.$ $2.02$ $×$ ${10}^{4}$
$2.$ $3.14$ $×$ ${10}^{3}$
$3.$ $2.02$ $×$ ${10}^{-4}$
$4.$ $1.01$ $×$ ${10}^{-4}$

Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The ionization constants of HCOOH, and HCN at 298K are 1.8 × 10–4 and 4.8 × 10–9 respectively. The ionization constants of the corresponding conjugate bases of HCOOH and HCN will be

 1 5.6 × 10–11, 2.08 × 10–6 2 2.4 × 10–11, 4.2 × 10–6 3 3.5 × 10–11, 1.7 × 10–6 4 4.2 × 10–11, 1.2 × 10–6
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The ionization constant of phenol is 1.0 × 10–10. The concentration of phenolate ion in 0.05 M solution of phenol will be:

 1 4.2 × 10–4 M 2 3.6 × 10–5 M 3 7.8 × 10–6 M 4 2.2 × 10–6 M
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The first ionization constant of H2S is 9.1 × 10–8. The concentration of HS ion in its 0.1 M solution will be:

 1 12.3 × 10–7 M 2 11.4 × 10–6 M 3 3.5 × 10–4 M 4 9.54 × 10–5 M
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The ionization constant of acetic acid is 1.74 × 10–5. The pH of acetic acid in its 0.05 M solution will be:
1. 7.81

2. 3.03

3. 8.54

4. 1.45

Subtopic:  Ionisation Constant of Acid, Base & Salt | pH calculation |
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The ionization constant of propanoic acid is 1.32 × 10–5. The degree of ionization of 0.05M acid solution will be:

1. $\mathrm{\alpha }$ 0.63 × 102

2. $\mathrm{\alpha }$ 1.63 × 104

3. $\mathrm{\alpha }$ 1.63 × 102

4. $\mathrm{\alpha }$ 0.05 × 102

Subtopic:  Ionisation Constant of Acid, Base & Salt | pH calculation |
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