The compound with the highest pH among the following is:

1. CH₃COOK

2. Na₂CO₃

3. NH₄Cl

4. NaNO₃

At 25 ºC, the dissociation constant of a base, BOH, is 1.0 × 10^–12. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:

The pK_b of dimethylamine and pk_a of acetic acid are 3.27 and 4.77 respectively at T (K).
The correct option for the pH of dimethylammonium acetate solution is:

For the equilibrium,

2NOCl(g) $\leftrightharpoons$2NO(g) + Cl₂(g) the value of the equilibrium constant, K_c is 3.75 × 10^–6 at 1069 K. What is the value of K_p​ for the reaction at this temperature?

1. 0.048

2. 0.67

3. 0.29

4. 0.033

Hydrolysis of sucrose gives,

Sucrose + H₂O  $\leftrightharpoons$Glucose + Fructose

The equilibrium constant K_c for the reaction is 2 ×10¹³ at 300K. The value of ∆G^⊖ at 300K is:

1. – 5.64 ×10⁴ J mol^–1
2. – 7.64 ×10⁴ J mol^–1
3. – 6.64 ×10⁴ J mol^–1
4. – 8.64 ×10⁴ J mol^–1

The ionization constant of the hypochlorous acid is 2.5 × 10^–5. The concentration of hypochlorous acid 0.08 M. The percent dissociation of HOCl is:

1. 2.56 %
2. 1.21 %
3. 1.76 %
4. 2.21 %

The solubility of A₂X₃ in pure water, assuming that neither kind of ion reacts with water is:
(solubility product of A₂X₃, K_sp = 1.1 × 10^–23)

The salt solution that is basic in nature is: 

1. Ammonium chloride.

2. Ammonium sulphate.

3. Ammonium nitrate.

4. Sodium acetate.

For the given reaction:
H₂NCOONH₄ (s) \( \rightleftharpoons\) 2NH₃ (g) + CO₂ (g),
total pressure at equilibrium is found to be 18 atmospheres. The value of K_p for the above equilibrium will be:

1. 72 atm³

2. 144 atm³

3. 432 atm³

4. 864 atm³

At 4^oC , ionic product of water (K\(\omega\)) is 10^-16 . At this temperature, a solution has pH = 7.5 . The nature of this solution at 4^oC will be 

1. Acidic 

2. Alkaline 

3. Neutral

4. Cannot be predicted