Q. No.| Statement I: | According to Lewis's concept, H2O acts as an amphoteric substance. |
| Statement II: | H2O act as an acid on reaction with NH3, while it acts as a base on reaction with H2S. |
| 1. | Both Statement I and Statement II are correct. |
| 2. | Both Statement I and Statement II are incorrect. |
| 3. | Statement I is correct and Statement II is incorrect. |
| 4. | Statement I is incorrect and Statement II is correct. |
Then, the ratio of \(\frac{[CH_3CH_2COO^-]}{[CH_3CH_2COOH]}\) is-
(Given \(K_a=10^{-5} \))
1. 0.1
2. 10
3. 0.2
4. 20
The solubility of Ca(OH)2 in water is:
[Given: Ksp Ca(OH)2 in water = 5.5 × 10–6]
1. 1.77 × 10–6
2. 1.11 × 10–6
3. 1.11 × 10–2
4. 2.77 × 10–2
The pH of an ammonium phosphate solution, if the pKa of phosphoric acid and the pKb of ammonium
hydroxide are 5.23 and 4.75 respectively, is:
| 1. | 8 | 2. | 6 |
| 3. | 7 | 4. | 10 |
| Assertion (A): | When Cu (II) and sulphide ions are mixed, they react together extremely quickly to give a solid. |
| Reason (R): | The equilibrium constant of Cu2+(aq) + S2- (aq) ⇋ CuS(s) is high because the solubility product is low. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A) |
| 2. | Both (A) and (R) are False. |
| 3. | (A) is True but (R) is False. |
| 4. | Both (A) and (R) are True but (R) is not the correct explanation of (A) |
An acidic buffer is obtained on mixing :
1. 100 mL of 0.1 M CH3COOH and 100 mL of 0.1 M NaOH.
2. 100 mL of 0.1 M HCl and 200 mL of 0.1 M NaCl.
3. 100 mL of 0.1 M HCl and 200 mL of 0.1 M CH3COONa.
4. 100 mL of 0.1 M CH3COOH and 200 mL of 0.1 M NaOH.
100 mL of 0.1 M HCl is taken in a beaker and to it 100 mL of 0.1 M NaOH is added in steps of 2 mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?
| 1. |  |
2. |  |
| 3. |  |
4. |  |
At 1990 K and 1 atm pressure, there are an equal number of Cl2 molecules and Cl atoms in the reaction mixture.
The value of KP for the reaction under the above conditions is x × 10–1. The value of x is:
1. 4
2. 8
3. 5
4. 10
For the reaction A(g)(B)(g), the value of the equilibrium constant at 300 K and 1 atm is equal to 100.0. The value of rG for the reaction at 300 K and 1 atm in J mol–1 is – xR, where x is:
(R = 8.31 J mol–1 K–1 and ln 10 = 2.3)
1. 1400
2. 1380
3. 1360
4. 1340
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