If a solution of 0.1 M NH₄OH and 0.1 M NH₄Cl has pH 9.25, then the pK_b of NH₄OH will be:

1.	9.25	2.	4.75
3.	3.75	4.	8.25

Among the following , the compound with highest pH is : 

1. CH₃COOK

2. Na₂CO₃ 

3. NH₄Cl

4. NaNO₃

The sharp pH change near the equivalence point in acid-base titration enables indicator detection. Which of the following equations correctly explains the pH change based on the concentration ratio of an indicator's conjugate acid (HIn) and base (In⁻) forms?

Solubility of a M₂S salt is $3.5\times {10}^{-6}$ then find out solubility product.

1. $1.7\times {10}^{-6}$

2. $1.7\times {10}^{-16}$

3. $1.7\times {10}^{-18}$

4. $1.7\times {10}^{-12}$

Find Ksp of an MX₂ type electrolyte if its solubility is 0.5 × 10⁻⁴ mol L⁻¹.

1. $5\times {10}^{-12}$

2. $25\times {10}^{-10}$

3. $1\times {10}^{-13}$

4. $5\times {10}^{-13}$

If the solubility product of a sparingly soluble salt AX₂ is $3.2\times {10}^{-11}$ , find its solubility (in mol L^–1):

What is the degree of ionization of an acid solution with a concentration of 0.005 M and a pH of 5?
 

1. $0.1\times {10}^{-2}$

2. $0.2\times {10}^{-2}$

3. $0.5\times {10}^{-4}$

4. $0.6\times {10}^{-6}$

Which among the following acids is the strongest, based on their given pKa values?

(I) 4.0

(II) 3.5

(III) 2.5

(IV) 2.0

1. I.0

2. II

3. III

4. IV

A solution has hydrogen ion concentration 0.0005 M, its pOH is:

1. 8.2798

2. 10.6990

3. 12.7854

4. 13.3344

At 25°C, the pH of a solution containing 0.10 M sodium acetate and 0.03 M acetic acid will be:

[pK_a value of ${\mathrm{CH}}_3\mathrm{COOH}=4.57$]

1. 3.24

2. 4.59

3. 5.09

4. 6.67