For the following reaction, 
 H$$₂(g)+I₂(g)⇌2HI(g) $at$ $250°C,$

The effect on the state of equilibrium on doubling the volume of the system will be:

1.	Shift to the reactant side	2.	Shift to the product side
3.	No effect on the state of equilibrium	4.	Liquefaction of HI

Which of the following cannot act as a buffer? 
1. NaH₂PO₄ + H₃PO₄
2. NH₄OH + NH₄CI
3. NaOH + CH₃COONa
4. Both (1) & (3)

If the pH of 0.1 M NaCN solution is 11, then the percentage hydrolysis will be:

1. 0.1%

2. 1%

3. 0.01%

4. 10%

How much water should be added to 400 mL of HCI solution in order to raise the pH by one unit?

In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be:

The degree of hydrolysis of the salt is independent of the concentration of a solution: 
1. NH₄CI
2. NH₄CN
3. (NH₄)₂SO₄
4. All of the above

The dissociation of solid ${\mathrm{NH}}_4\mathrm{SH}$ in a closed container produces a pressure of 4 atm at $95°\mathrm{C}$, then ${\mathrm{K}}_{\mathrm{p}}$ for the reaction will be:

${\mathrm{NH}}_4\mathrm{SH}\left(\mathrm{s}\right)\stackrel{}{\rightleftharpoons }{\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

The number of ${\mathrm{H}}^{\oplus }$ ions present in 1 ml of a solution whose pH= 4 , is given as:

($N_A=$ $Avogadro\text{'}s$ $number$)

1. ${10}^{-7}{N}_A$

2. ${10}^{-8}{N}_A$

3. ${10}^{-16}{N}_A$

4. ${10}^{-14}{N}_A$

If the pH of an acidic buffer is 5.7 and ${\mathrm{pK}}_{\mathrm{a}}$ is 5 then the ratio of $\frac{\left[\mathrm{Salt}\right]}{\left[\mathrm{Acid}\right]}$ will be:

On adding NH₄CI to an NH₄OH solution, the pH of the solution will