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The solubility of \(Sr(OH)_2 \) at 298 K is 20 g/L of solution. The pH of this solution will be:
(Given: molar mass of Sr = 88 g/mol; log 40 =1.60 ; and log 122 = 2.086)
1. 13.51
2. 0.48
3. 10.22
4. 11.25
Subtopic: Solubility Product |
77%
Level 2: 60%+
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Select the correct order of solubility of AgCl in the following solutions:
(a) \(0.1 \text {M NaCl (aq)} \)
(b) \(0.1~ \text {M} ~\text {CaCl}_2 ~ (\text {aq}) \)
(c) \(0.1~ \text {M} ~\text {AlCl}_3 ~ (\text {aq}) \)
1. (a) = (b) = (c)
2. (a) > (b) > (c)
3. (a) < (b) < (c)
4. (c) > (b) = (a)
(a) \(0.1 \text {M NaCl (aq)} \)
(b) \(0.1~ \text {M} ~\text {CaCl}_2 ~ (\text {aq}) \)
(c) \(0.1~ \text {M} ~\text {AlCl}_3 ~ (\text {aq}) \)
1. (a) = (b) = (c)
2. (a) > (b) > (c)
3. (a) < (b) < (c)
4. (c) > (b) = (a)
Subtopic: Common Ion Effect |
68%
Level 2: 60%+
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The solubility of BaSO4 in 10-3 M H2SO 4 solution will be:
(Given: Ksp for BaSO4 = 1.1 × 10-10)
(Given: Ksp for BaSO4 = 1.1 × 10-10)
| 1. | 1.1 × 10–13 M | 2. | 1.1 × 10–7 M |
| 3. | 5.5 × 10–7 M | 4. | 5.5 × 10–8 M |
Subtopic: Solubility Product |
84%
Level 1: 80%+
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If 0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is:
| 1. | 3 | 2. | 2 |
| 3. | 4 | 4. | 1 |
Subtopic: pH calculation |
70%
Level 2: 60%+
NEET - 2022
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Accumulation of lactic acid (HC3H5O3 a monobasic acid), in tissues leads to pain and fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociated. The value of the dissociation constant, Ka, for this acid, will be:
1. 1.4 × 10–5
2. 1.4 × 10–4
3. 3.7 × 10–4
4. 2.8 × 10–4
1. 1.4 × 10–5
2. 1.4 × 10–4
3. 3.7 × 10–4
4. 2.8 × 10–4
Subtopic: Ionisation Constant of Acid, Base & Salt |
71%
Level 2: 60%+
NEET - 2013
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At 100 °C the Kw of water is 55 times its value at 25ºC. What will be the pH of a neutral solution?
(log 55 = 1.74)
(log 55 = 1.74)
| 1. | 7.00 | 2. | 7.87 |
| 3. | 5.13 | 4. | 6.13 |
Subtopic: pH calculation |
56%
Level 3: 35%-60%
NEET - 2013
Hints
The dissociation constant of a weak acid is \(1\times 10^{-4}\) in order to prepare a buffer solution with pH=5 the [salt]/ [Acid] ratio should be:
| 1. | 4 : 5 | 2. | 10 : 1 |
| 3. | 5 : 4 | 4. | 1 : 10 |
Subtopic: Buffer |
73%
Level 2: 60%+
NEET - 2013
Hints
Consider the following statements regarding the pH of the solution at the equivalence point when a weak acid is titrated with a weak base?
The correct statements are :
| (i) | pH depends on the concentration of acid and base. |
| (ii) | pH is independent of the concentration of acid and base. |
| (iii) | pH depends on pKa of acid and pKb of the base. |
| (iv) | pH is independent of pKa of acid and pKb of base. |
The correct statements are :
| 1. | only (i) and (iii) | 2. | only (i) and (iv) |
| 3. | only (ii) and (iii) | 4. | only (ii) and (iv) |
Subtopic: pH calculation |
57%
Level 3: 35%-60%
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Initially 2 moles of \(NOCl \) taken in 1 L of closed container and it dissociates into NO and Cl2 gas.
The reaction is as follows:
\(2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_2(g)\)
Calculate the equilibrium constant Kc given that 0.4 moles of NO is obtained at equilibrium.
The reaction is as follows:
\(2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_2(g)\)
Calculate the equilibrium constant Kc given that 0.4 moles of NO is obtained at equilibrium.
| 1. | 142 × 10-4 | 2. | 142 × 10-6 |
| 3. | 125 × 10-4 | 4. | 130 × 104 |
Subtopic: Introduction To Equilibrium |
85%
Level 1: 80%+
JEE
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Given below are two statements:
| Assertion (A): | If Qp<Kp, reaction moves in the direction of reactants. |
| Reason (R): | The reaction quotient is defined in the same way as the equilibrium constant at any stage of the reaction. |
| 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. |
Subtopic: Introduction To Equilibrium |
76%
Level 2: 60%+
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