Q. No.
Assertion (A):
For the reaction: H2(g) + I2(g) \(\rightleftharpoons\) 2HI(g), if the volume of the vessel is reduced to half of its original volume, the equilibrium concentration of all gases will be doubled.
Reason (R):
According to Le-Chatelier's principle, reaction shifts in a direction that tends to minimize the effect of stress.
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.
| Assertion (A): | Salts of strong acid and strong base do not undergo hydrolysis. |
| Reason (R): | These salts undergo hydration. |
| 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. |
[Given: pKa = 4.75]
1. 5.05
2. 4.15
3. 5.35
4. 4.75
| Assertion (A): | The solubilities of two sparingly soluble salts, Ni(OH)2 and AgCN with a Ksp of \(4 \times 10^{-8} ~and~1 \times 10^{-10}~mol/L\)respectively. |
| Reason (R): | AgCN is less soluble than Ni(OH)2 |
| 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. |
| 1. | \(NaCl\) | 2. | \(CH_3COONH_4\) |
| 3. | \(Na_2SO_4 \) | 4. | None of these |
1. 0.25 Mol/L
2. \({1 \over 22.4 } Mol /L\)
3. 0.175 Mol/L
4. \({ 1 \over 5.6}~ Mol / L\)
1. 1.84
2. 2.90 × 10−3
3. 1.81 × 10−6
4. 7.56 × 10−23
What can be the active mass of CaCO3 if 10 grams of CaCO3 are taken in a one-liter container?
[Given: Molecular weight of CaCO3 = 100]
1. 0.1
2. 1
3. 0.01
4. 10
The pH of 10-6 M CH3COOH will be:
(Given: ka of CH3COOH = 1.8 \(\times\) 10-5 & log 4.24 =0.63)
1. 5.37
2. 7.0
3. Slightly more than 6
4. 6.95
A buffer solution is defined as a solution whose pH remains practically constant even when small amounts of an acid or a base are added to it.
Henderson's equation is used to determine pH of buffer mixtures of different types:
For acidic buffer, Henderson's equation is :
pH= pKa + log \([Salt] \over [Acid]\) (ka = ionisation constant of weak acid)
For basic buffer, Henderson's equation is :
POH = Pkb + log \([Salt] \over [Base]\) (kb = ionisation constant of weak base)
How many moles of HCl are required with 0.01 mole NaCN to prepare a buffer solution of pH =9?
[Given: Ka of HCN = \(1 \times 10^{-10}\)]
1. 0.009
2. 0.09
3. 0.9
4. Buffer solution cannot formed
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