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Q. No.Consider the following statements regarding the pH of the solution at the equivalence point when a weak acid is titrated with a weak base?
(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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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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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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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
(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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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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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
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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
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