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:

1.	1.90	2.	13.42
3.	1.47	4.	12.63

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). 

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

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

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

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

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

The pH of neutral water at this temperature will be:

What will be the pH of a 0.1 M chloroacetic acid solution with an ionization constant of 1.35 × 10^–3?

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

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

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

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

The percentage ionization of 0.02 M dimethylamine solution if it also contains 0.1 M NaOH solution (K_b of dimethylamine = 5.4 × 10^–4) will be:

The degree of ionization of 0.05 M acetic acid is:

(pK_a = 4.74)