The salt solution that is basic in nature is: 

1. Ammonium chloride.

2. Ammonium sulphate.

3. Ammonium nitrate.

4. Sodium acetate.

The solubility product for a salt of type AB is $4\times {10}^{-8}$.  The molarity of its standard solution will be:
1. $2\times {10}^{-4}$ $\mathrm{mol}/\mathrm{L}$

2. $16\times {10}^{-16}$ $\mathrm{mol}/\mathrm{L}$

3. $2\times {10}^{-16}$ $\mathrm{mol}/\mathrm{L}$

4. $4\times {10}^{-4}$ $\mathrm{mol}/\mathrm{L}$

The maximum concentration of equimolar solutions, of ferrous sulphate and sodium sulphide, so that when mixed in equal volumes, there is no precipitation of iron sulphide, will be :

(For iron sulphide, K_sp = 6.3 × 10^–18). 

$1.$ $5.02$ $\times {10}^{-9}$ $\mathrm{M}$

$2.$ $5.02$ $\times$ ${10}^9$ $\mathrm{M}$

$3.$ $2.$ $25$ $\times$ ${10}^{-13}$ $\mathrm{M}$

$4.$ $\mathrm{Can}\text{'}\mathrm{t}$ $\mathrm{predict}$

A mixture of 10 mL of 0.2 M Ca(OH)2 and 25 mL of 0.1 M HCl is prepared. The pH of the resultant mixture would be:

The ionic product of water at 310 K is 2.7 × 10^–14.

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

1. 2.56

2. 6.14

3. 7.96

4. 11.74

The pH of a 0.1 M solution of cyanic acid (HCNO) is 2.34. The ionization constant of the acid will be:

$1.$ $2.02$ $\times$ ${10}^4$
$2.$ $3.14$ $\times$ ${10}^3$
$3.$ $2.02$ $\times$ ${10}^{-4}$
$4.$ $1.01$ $\times$ ${10}^{-4}$

At 298 K, the solubility of Sr(OH)₂ is 19.23 g/L. The pH of the solution will be:

0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. The pH of the solution will be