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Q. No.Which combination of the following substances will result in the formation of an acidic buffer when mixed?
1.
Weak acid and it's salt with a strong base.
2.
Equal volumes of equimolar solutions of weak acid and weak base.
3.
Strong acid and its salt with a strong base.
4.
Strong acid and its salt with a weak base.
(The pKa of acid = pKb of the base)
(The pKa of acid = pKb of the base)
Subtopic: Buffer |
78%
Level 2: 60%+
NEET - 2023
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For a weak acid HA, the percentage of dissociation is nearly 1% at equilibrium.
If the concentration of acid is 0.1 mol L-1, then the correct option for its Ka at the same temperature will be:
If the concentration of acid is 0.1 mol L-1, then the correct option for its Ka at the same temperature will be:
| 1. | \(1 \times 10^{-4}\) |
| 2. | \(1 \times 10^{-6} \) |
| 3. | \(1 \times 10^{-5} \) |
| 4. | \(1 \times 10^{-3} \) |
Subtopic: Ionisation Constant of Acid, Base & Salt |
68%
Level 2: 60%+
NEET - 2023
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The term chemical equilibrium applies to a system:
| 1. | where the forward and reverse reactions have stopped. |
| 2. | whose rate law is of zero order. |
| 3. | where individual molecules are still reacting, but there is no net change in the system. |
| 4. | in which all components are in the same phase. |
Subtopic: Introduction To Equilibrium |
85%
Level 1: 80%+
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If the following endothermic reaction is at equilibrium in a rigid reaction vessel,
CH4 (g) + H2O(g) \(\rightleftharpoons\) CO(g) + 3 H2 (g)
then which one of the following changes would cause the equilibrium to shift to the right?
1. Adding Ne(g).
2. Removing some H2O(g).
3. Increasing the pressure.
4. Increasing the temperature.
CH4 (g) + H2O(g) \(\rightleftharpoons\) CO(g) + 3 H2 (g)
then which one of the following changes would cause the equilibrium to shift to the right?
1. Adding Ne(g).
2. Removing some H2O(g).
3. Increasing the pressure.
4. Increasing the temperature.
Subtopic: Le Chatelier's principle |
80%
Level 1: 80%+
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The value of the solubility product for copper(I) chloride is Ksp = 1.2 × 10−6. Under normal conditions, the maximum concentration of an aqueous CuCl solution will be:
1. Less than 10−6 M.
2. Greater than 10−6 M and less than 10−4 M.
3. Greater than 10−4 M and less than 102 M.
4. Greater than 10−2 M and less than 10−1 M.
1. Less than 10−6 M.
2. Greater than 10−6 M and less than 10−4 M.
3. Greater than 10−4 M and less than 102 M.
4. Greater than 10−2 M and less than 10−1 M.
Subtopic: Solubility Product |
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Level 2: 60%+
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Given the following equilibrium:
N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g), ∆H = −91.8 kJ
How would an increase in temperature affect the concentration of N2 at equilibrium?
1. The concentration of N2 will increase because of an increase in Keq.
2. The concentration of N2 will decrease because of an increase in Keq.
3. The concentration of N2 will increase because of a decrease in Keq.
4. The concentration of N2 will remain unchanged.
N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g), ∆H = −91.8 kJ
How would an increase in temperature affect the concentration of N2 at equilibrium?
1. The concentration of N2 will increase because of an increase in Keq.
2. The concentration of N2 will decrease because of an increase in Keq.
3. The concentration of N2 will increase because of a decrease in Keq.
4. The concentration of N2 will remain unchanged.
Subtopic: Le Chatelier's principle |
65%
Level 2: 60%+
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If Ksp of KI is 1.45 × 10−6 in propanol at 25°C, what would Ksp of KI be in propane at the same temperature?
1. 1.84
2. 2.90 × 10−3
3. 1.81 × 10−6
4. 7.56 × 10−23
1. 1.84
2. 2.90 × 10−3
3. 1.81 × 10−6
4. 7.56 × 10−23
Subtopic: Solubility Product |
Level 3: 35%-60%
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The molecule that can behave as a Bronsted-Lowry acid but not a Lewis acid is:
1. CF4
2. NaAlCl4
3. HF
4. Br2
1. CF4
2. NaAlCl4
3. HF
4. Br2
Subtopic: Ionisation Constant of Acid, Base & Salt |
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Which of the following acids will dissociate to the greatest extent (in water)?
1. HCN (hydrocyanic acid), Ka = 6.2 × 10−10
2. HNCO (cyanic acid), Ka = 3.3 × 10−4
3. HClO (hypochlorous acid), Ka = 2.9 × 10−8
4. HBrO (hypobromous acid), Ka = 2.2 × 10−9
1. HCN (hydrocyanic acid), Ka = 6.2 × 10−10
2. HNCO (cyanic acid), Ka = 3.3 × 10−4
3. HClO (hypochlorous acid), Ka = 2.9 × 10−8
4. HBrO (hypobromous acid), Ka = 2.2 × 10−9
Subtopic: Ionisation Constant of Acid, Base & Salt |
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The equilibrium concentration of the species in the reaction \(A+B \rightleftharpoons C+D\) are 2, 3, 10 and 6 mol L–1, respectively at 300 K. \(\Delta G^o\) for the reaction is: (R = 2 cal/mol K)
| 1. | –13.73 cal | 2. | 1372.60 cal |
| 3. | –137.26 cal | 4. | –1381.80 cal |
Subtopic: Introduction To Equilibrium |
73%
Level 2: 60%+
NEET - 2023
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