Find out the solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in 0.1 M NaOH, given that the ionic product of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ is 2x ${10}^{-\mathrm{15 }}$

1. 2 x ${10}^{-8}$ M.

2. 1 x ${10}^{-13}$ M

3. 1 x ${10}^8$ M 

4. 2 x ${10}^{-13}$ 

Which of the following salt solutions is basic in nature?

1. Ammonium chloride

2. Ammonium sulphate

3. Ammonium nitrate

4. Sodium acetate

The molar solubility of ${\mathrm{CaF}}_2 ({\mathrm{K}}_{\mathrm{sp}}=5.3 \mathrm{x} {10}^{-11})$ in 0.1 M solution of NaF will be:

1. $5.3 \mathrm{x} {10}^{-11} \mathrm{mol} {\mathrm{L}}^{-1}$

2. $5.3 \mathrm{x} {10}^{-8} \mathrm{mol} {\mathrm{L}}^{-1}$

3. $5.3 \mathrm{x} {10}^{-9} \mathrm{mol} {\mathrm{L}}^{-1}$

4. $5.3 \mathrm{x} {10}^{-10} \mathrm{mol} {\mathrm{L}}^{-1}$

Which of the following cannot act both as a Bronsted acid and as a Bronsted base?

1. $HC{O}_3^{-}$

2. ${\mathrm{NH}}_3$

3. HCl

4. $HS{O}_4^{-}$

The pH of a 0.01 M NaOH (aq) solution will be:

1. 7.01

2. 2

3. 12

4. 9

Given that the equilibrium constant for the reaction 

$2S{O}_{2\left(g\right)} + O_{2\left(g\right)} \leftrightharpoons 2S{O}_{3\left(g\right) }$

has a value of 278 at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be:

$S{O}_{3\left(g\right)} \leftrightharpoons S{O}_{2\left(g\right) }+ 1/2 O_{2\left(g\right) }$

1.  $3.6 \times {10}^{-3}$

2.  $6.0 \times {10}^{-2}$

3.  $1.3 \times {10}^{-5}$

4.  $1.8 \times {10}^{-3}$

Given reaction: $A_{2\left(g\right)} + B_{2\left(g\right) }\leftrightharpoons 2A{B}_{\left(g\right) }$

At equilibrium , the concentrations of ${\mathrm{A}}_2 = 3.0 \times {10}^{-3} \mathrm{M} ; {\mathrm{B}}_2 = 4.2 \times {10}^{-3} \mathrm{M} \mathrm{and} \mathrm{AB} = 2.8 \times {10}^{-3} \mathrm{M}$

If the reaction takes place in a sealed vessel at $527°C$, then the value of $K_C$ will be : 

1.  3.9 

2.  0.6 

3.  4.5

4.  2.0 

In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag⁺
and Pb²⁺ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl– concentration is 0.10 M. What will the concentration of Ag⁺
and Pb²⁺ at equilibrium?

$$\begin{gathered} \left({\mathrm{K}}_{\mathrm{sp}} \mathrm{for} \mathrm{AgCl}=1.8\times {10}^{-10}\right) \\ (K_{sp} for PbC{l}_2=1.7\times {10}^{-5}) \end{gathered}$$

1. $\left[A{g}^{+}\right]=1.8\times {10}^{-11} M;$

    $\left[P{b}^{2+}\right]=1.7\times {10}^{-4}M$

2. $\left[A{g}^{+}\right]=1.8\times {10}^{-7} M;$

    $\left[P{b}^{2+}\right]=1.7\times {10}^{-6}M$

3. $\left[A{g}^{+}\right]=1.8\times {10}^{-11} M;$

   $\left[P{b}^{2+}\right]=8.5\times {10}^{-5}M$

4. $\left[A{g}^{+}\right]=1.8\times {10}^{-9} M;$

   $\left[P{b}^{2+}\right]=1.7\times {10}^{-3}M$

The reaction

$2A+B\left(g\right) \rightleftharpoons 3C\left(g\right)+D\left(g\right)$

begins with the concentrations of A and B both at an intial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression.

1. $\left[{(0.75)}^3\right(0.25\left)\right]÷\left[{(0.50)}^2\right(0.75\left)\right]$

2. $\left[{(0.75)}^3\right(0.25\left)\right]÷\left[{(0.50)}^2\right(0.25\left)\right]$

3. $\left[{(0.75)}^3\right(0.25\left)\right]÷\left[{(0.75)}^2\right(0.25\left)\right]$

4. $\left[{(0.75)}^3\right(0.25\left)\right]÷\left[{(1.00)}^2\right(1.00\left)\right]$

The equilibrium constant Kp for the following reaction is-

${{\mathrm{MgCO}}_3}_{\left(\mathrm{s}\right)}\rightleftharpoons {\mathrm{MgO}}_{\left(\mathrm{s}\right)}+{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$

1. $\mathrm{Kp}={\mathrm{P}}_{{\mathrm{CO}}_2}$

2. $\mathrm{Kp}={\mathrm{P}}_{{\mathrm{CO}}_2}\times \frac{{\mathrm{P}}_{{\mathrm{CO}}_2}\times {\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}$

3. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{CO}}_2}+{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}$

4. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}{{\mathrm{P}}_{{\mathrm{CO}}_2}\times {\mathrm{P}}_{\mathrm{MgO}}}$