An incorrect statement about equilibrium among the following is:

1.	Equilibrium is possible only in a closed system at a constant temperature.
2.	All measurable properties of the system remain constant.
3.	All the physical processes stop at equilibrium.
4.	The opposing processes occur at the same rate and there is a dynamic but stable condition.

The salt solution that is basic in nature is: 

1. Ammonium chloride.

2. Ammonium sulphate.

3. Ammonium nitrate.

4. Sodium acetate.

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 compound with the highest pH among the following is:

1. CH₃COOK

2. Na₂CO₃

3. NH₄Cl

4. NaNO₃

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 concentration of $\left[{\mathrm{H}}^{+}\right]$ ion in a solution containing 0.1 M HCN and 0.2 M NaCN will be:

(${\mathrm{K}}_{\mathrm{a}}$ for HCN = $6.2\times {10}^{-10}$)

1. 3.1$\times {10}^{10}$

2. $6.2\times {10}^5$

3.$$ $6.2\times {10}^{-10}$

4. $3.1\times {10}^{-10}$