At 4oC , ionic product of water (K\(\omega\)) is 10-16 . At this temperature, a solution has pH = 7.5 . The nature of this solution at 4oC will be
1. Acidic
2. Alkaline
3. Neutral
4. Cannot be predicted
For the given reaction: H2NCOONH4 (s) \( \rightleftharpoons\) 2NH3 (g) + CO2 (g),
total pressure at equilibrium is found to be 18 atmospheres. The value of Kp for the above equilibrium will be
1. 72 atm3
2. 144 atm3
3. 432 atm3
4. 864 atm3
Assertion (A): | Sparingly soluble salts AB and XY2 with the same solubility product, will have different solubility. |
Reason (R): | Solubility of sparingly soluble salt depend upon solubility product as well as the type of salt. |
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. | Y has a hydrogen ion concentration 2 times greater than X. |
2. | X has a hydrogen ion concentration 100 times greater than Y. |
3. | X has a hydrogen ion concentration 4 times greater than Y |
4. | Y has a hydrogen ion concentration 100 times greater than X |
1. | CH3OH is the conjugate acid of CH3O-. |
2. | The CH3O– ion is a Lewis acid. |
3. | The final mixture of solutions would have a pH below 7. |
4. | Water is acting as a Bronsted–Lowry base. |
The solubility of A2X3 in pure water, assuming that neither kind of ion reacts with water is:
(solubility product of A2X3, Ksp = 1.1 × 10–23)
1. | 5.0 × 10–5 mol/L. | 2. | 1.0 × 10–5 mol/L |
3. | 1.0 × 10–4 mol/L | 4. | 5.0 × 10–4 mol/L. |