pH of 0.005M calcium acetate (pk_a of CH₃COOH = 4.74) is: 

${\mathrm{K}}_{\mathrm{a}}$ for ${\mathrm{CH}}_3\mathrm{COOH}$ is $1.8\times {10}^{-5}$ and K_b for ${\mathrm{NH}}_4\mathrm{OH}$ is $1.8\times {10}^{-5}$. The pH of ammonium acetate will be: 

1. 7.005

2. 4.75

3. 7.0

4. Between 6 and 7

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:

The salt solution that is basic in nature is: 

1. Ammonium chloride.

2. Ammonium sulphate.

3. Ammonium nitrate.

4. Sodium acetate.

A 0.02 M solution of pyridinium hydrochloride has a pH of 3.44. The ionization constant of pyridine will be:

The ionization constant of nitrous acid is 4.5 × 10^–4.  The pH of a 0.04 M sodium nitrite solution will be:

The ionization constant of chloroacetic acid is 1.35 × 10^–3. The pH of a 0.1 M acid solution will be:

The salt that gives a neutral solution in water is: