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Q. No.The pH of a 0.045 M solution of the monoprotic acid is 5.30. What is the Ka of monoprotic acid?
(Given: 10-5.30 = \(5.0 \times 10^{-6}\))
1. 1.1 × 10-4
2. 5.0 × 10-6
3. 2.0 × 10-9
4. 5.6 × 10-10
Subtopic: Ionisation Constant of Acid, Base & Salt |
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What is the correct equilibrium expression for the given reaction?
Cu(OH)2(s) + 4 NH3(aq) \(\leftrightharpoons\) Cu(NH3)42+(aq) + 2 OH¯(aq)
Cu(OH)2(s) + 4 NH3(aq) \(\leftrightharpoons\) Cu(NH3)42+(aq) + 2 OH¯(aq)
| 1. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][OH^-]}{[NH_3]}\) |
| 2. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][2~OH^-]}{[4~NH_3]}\) |
| 3. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][OH^-]^2}{[NH_3]^4}\) |
| 4. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][2~OH^-]^2}{[4~NH_3]^4}\) |
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the following statements:
| I. | Ionic product of water KW cannot change with temperature. |
| II. | The value of the equilibrium constant is independent of the initial concentration of the reactant and products. |
| III. | The equilibrium constant for an exothermic reaction decreases as the temperature increases. |
Which of the above statements is true?
1. I and II only
2. I and III only
3. II and III only
4. I, II, and III
Subtopic: Introduction To Equilibrium |
82%
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| Assertion(A): | \(Ni(s)+4CO(g)\rightleftharpoons Ni(CO)_4(g)\\ \text{For above reaction,}\\ K_C=\frac{[Ni(CO)_4]}{[CO]^4}\) |
| Reason(R): | For heterogeneous equilibrium, the concentrations of pure solids or liquids are not considered in the expression of an equilibrium constant. |
| 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. | Both (A) and (R) are false. |
Subtopic: Introduction To Equilibrium |
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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:
| 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%
From NCERT
NEET - 2023
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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) |
Subtopic: Buffer |
78%
From NCERT
NEET - 2023
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Amongst the given option which of the following molecules/ion acts as a Lewis acid?
1. \(\text{OH}^- \)
2. \(\text{NH}_3 \)
3. \(\text H_2 \text O \)
4. \(\text{BF}_3 \)
1. \(\text{OH}^- \)
2. \(\text{NH}_3 \)
3. \(\text H_2 \text O \)
4. \(\text{BF}_3 \)
Subtopic: Acids & Bases - Definitions & Classification |
76%
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NEET - 2023
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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
1. 4 : 5
2. 10 : 1
3. 5 : 4
4. 1 : 10
Subtopic: Buffer |
74%
From NCERT
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 |
60%
From NCERT
NEET - 2013
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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 |
72%
From NCERT
NEET - 2013
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NEET 2025 - Target Batch
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