The ionization constant of acetic acid is \(1.74 × 10^{–5}.\) The pH of acetic acid in its 0.05 M solution will be:
1. 7.81

2. 3.03

3. 8.54

4. 1.45

The ionization constant of propanoic acid is 1.32 × 10^–5. The degree of ionization of 0.05M acid solution will be:

1. $\mathrm{\alpha }$ = 0.63 × 10^–2

2. $\mathrm{\alpha }$ = 1.63 × 10^–4

3. $\mathrm{\alpha }$ = 1.63 × 10^–2

4. $\mathrm{\alpha }$ = 0.05 × 10^–2

The salt that gives a neutral solution in water is: 

${{\mathrm{I}}_2}_{\left(\mathrm{s}\right)}$ $+$ $5{{\mathrm{F}}_2}_{\left(\mathrm{g}\right)}$ $$ $\to 2{\mathrm{IF}}_{5\left(g\right)}$ $$

The first ionization constant of H₂S is 9.1 × 10^–8. The concentration of HS^– ion in its 0.1 M solution will be:

OH^– , F^– , H⁺ and BCl₃

For the given reaction: 

PCl_{5 (g)}  $\leftrightharpoons$PCl_{3 (g)} + Cl_{2 (g)}, ∆_rH° = 124.0 kJ mol^–1 and K_c = 8.3 $\times$ 10^-3 mol L^-1 at 473 K

The effect on K_c if (i) pressure is increased  and (ii) the temperature is increased will be, respectively-

1. (i) Will increase; (ii) will decrease

2. (i) Will decrease; (ii) will remain the same 

3. (i) Will remain the same; (ii) will increase

4. (i) will remain the same; (ii) Will decrease

(a) PCl_{5 (g)} $\leftrightharpoons$ PCl_{3 (g)} + Cl_{2 (g)}

(b) CaO _(s) + CO_{2 (g)} $\leftrightharpoons$  CaCO_{3 (s)}

(c) 3Fe _(s) + 4H₂O _(g) $\leftrightharpoons$ Fe₃O_{4 (s)} + 4H_{2 (g)}

The effect of an increase in the volume on the number of moles of products in the above-mentioned reactions would be, respectively:

1. a) Increase,  b) decrease, c) same

2. a) Decrease,  b) same, c) increase

3. a) Increase,  b) increase, c) same

4. a) Increase,  b) decrease, c) increase

What is the molarity of the standard solution if the solubility product for a salt of type AB is $4\times {10}^{-8}$?

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