What is the molar solubility of aluminum hydroxide (Al(OH)₃) in a 0.2 M sodium hydroxide (NaOH) solution?
[Given: Solubility product of Al(OH)₃ is 2.4 × 10^–24]

1. 3 × 10^–22
2. 3 × 10^–19
3. 12 × 10^–21
4. 12 × 10^–22

The molar solubility of Cd(OH)₂ is 1.84 × 10^–5 M in water. The expected solubility of Cd(OH)₂ in a buffer solution of pH = 12 is:

In which one of the following equilibria, K_p \(\ne\) K_C?

1. $2NO\left(g\right)\rightleftharpoons N_2\left(g\right)+O_2\left(g\right)$

2. $2C\left(s\right)+O_2\left(g\right)\rightleftharpoons 2CO\left(g\right)$

3. $2HI\left(g\right)\rightleftharpoons H_2\left(g\right)+I_2\left(g\right)$

4. $N{O}_2\left(g\right)+S{O}_2\left(g\right)\rightleftharpoons NO\left(g\right)+S{O}_3\left(g\right)$

An acidic buffer is obtained on mixing :
1. 100 mL of 0.1 M CH₃COOH and 100 mL of 0.1 M NaOH.
2. 100 mL of 0.1 M HCl and 200 mL of 0.1 M NaCl.
3. 100 mL of 0.1 M HCl and 200 mL of 0.1 M CH₃COONa.
4. 100 mL of 0.1 M CH₃COOH and 200 mL of 0.1 M NaOH.

If the equilibrium constant for $\mathrm{A}<mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace>\mathrm{B}<mspace\; width="1em"></mspace>+\hspace{0.17em}\mathrm{C}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}$ and that of $\mathrm{B}\hspace{0.17em}+\hspace{0.17em}\mathrm{C}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace>\mathrm{P}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}$, the equilibrium constant for $A<mspace\; width="1em"></mspace>\leftrightharpoons <mspace\; width="1em"></mspace>P$ is: 

1. ${\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}<mspace\; width="1em"></mspace>-<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}$

2. ${\mathrm{K}}_{\mathrm{eq}}^{(1)\hspace{0.17em}}\times <mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}$

3. ${\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}$

4. ${\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}<mspace\; width="1em"></mspace>/<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}$

100 mL of 0.1 M HCl is taken in a beaker and to it 100 mL of 0.1 M NaOH is added in steps of 2 mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?

1.		2.
3.		4.

Consider the following reaction 
\(\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g) ; \Delta H^0=+58 \mathrm{~kJ}\)
${}_{}$Also, consider the following stimuli on the above equilibrium.

For each of the above cases (I, II), the direction in which the equilibrium shifts is:
1. (I) Towards reactant, (II) No change.
2. (I) Towards product, (II) Towards reactant.
3. (I) Towards product, (II) No change.
4. (I) Towards reactant, (II) Towards product.

For a reaction; $X<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>Y<mspace\; width="1em"></mspace>\leftrightharpoons <mspace\; width="1em"></mspace>2Z$, 1.0 mol of X, 1.5 mol of Y and 0.5 mol of Z were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of Z was 1.0 mol L^–1 . The equilibrium constant of the reaction is $\frac{x}{15}$. The value of x is:

1. 24

2. 13

3. 16

4. 19

The solubility of Ca(OH)₂ in water is: 

[Given: K_sp Ca(OH)₂ in water = 5.5 × 10^–6]

1. 1.77 × 10^–6

2. 1.11 × 10^–6

3. 1.11 × 10^–2

4. 2.77 × 10^–2