Consider the following reaction:

${\mathrm{CO}}_{\left(\mathrm{g}\right)}$ $+$ $3{{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}$ $\rightleftharpoons$ ${{\mathrm{CH}}_4}_{\left(\mathrm{g}\right)}$ $$ $+$ ${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}$ $$

If the reaction mixture contains 0.30 mol of CO, 0.10 mol of H_2, and 0.02 mol of H₂O, and an unknown amount of CH₄ at equilibrium at 1300 K in a 1L flask, the concentration of CH₄ in the mixture will be -

(K_c = 3.90 at 1300 K) 

$1.$ $5.85$ $\times$ ${10}^2$ $\mathrm{M}$
$2.$ $5.85$ $\times$ ${10}^{-1}$ $\mathrm{M}$
$3.$ $5.85$ $\times$ ${10}^3$ $\mathrm{M}$
$4.$ $5.85$ $\times$ ${10}^{-2}$ $\mathrm{M}$

The concentration of hydrogen ion in a sample of soft drink is $3.8$ $\times {10}^{-3}$ $\mathrm{M}$. The  pH of the soft drink will be:

1. 3.14

2. 2.42

3. 11.58

4. 6.00

The pH of a sample of vinegar is 3.76. The concentration of H⁺ ions in the sample will be -

$1.$ $1.74$ $\times$ ${10}^{-4}$ $\mathrm{M}$
$2.$ $2.34$ $\times$ ${10}^{-11}\mathrm{M}$
$3.$ $2.86$ $\times$ ${10}^{-10}$ $\mathrm{M}$
$4.$ $1.74$ $\times$ ${10}^{-3}$ $\mathrm{M}$

The pH value of a 0.01 M solution of an organic acid is 4.15. The pK_a of the acid will be:

$1.$ $8.95$
$2.$ $1.43$
$3.$ $3.56$
$4.$ $6.30$

A solution containing 2 g of TlOH in 2 litres of water has a pH of?

(Atomic wt of Tl =204)

When 1mL of 13.6 M HCl is diluted with water to give 1 litre of solution, the pH of the resultant solution will be:

A 0.001 M aniline solution has a pH of:
(\(K_b = 4.27 \times 10^{-10}\))

The degree of ionization of 0.05 M acetic acid is:

(pK_a = 4.74)

$1.$ $1.91$ $\times {10}^{-2}$
$2.$ $2.46$ $\times$ ${10}^2$
$3.$ $1.93$ $\times$ ${10}^2$
$4.$ $2.34$ $\times$ ${10}^{-3}$

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 :

1. 0.54%

2. 0.05%

3. 5.40%

4. 54.00%

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