If the molar concentration of ${\mathrm{SnCl}}_4$ is $1.5$ $\times$ ${10}^{-3}$ mol L^–1, the concentration of chloride ions will be:

1.	3.0 x 10-3	2.	6.0 x 10-3
3.	0.3 x 10-3	4.	0.6 x 10-6

Given that the ionic product of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ is 2 × ${10}^{-\mathrm{15 }}$.
The solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in 0.1 M NaOH is ;

1. 2 × ${10}^{-8}$ M

2. 1 × ${10}^{-13}$ M

3. 1 × ${10}^8$ M 

4. 2 × ${10}^{-13}$ M

The concentration of $\left[{\mathrm{H}}^{+}\right]$ ion in a solution containing 0.1 M HCN and 0.2 M NaCN will be:

(${\mathrm{K}}_{\mathrm{a}}$ for HCN = $6.2\times {10}^{-10}$)

1. 3.1$\times {10}^{10}$

2. $6.2\times {10}^5$

3.$$ $6.2\times {10}^{-10}$

4. $3.1\times {10}^{-10}$

Which of the following change will shift the reaction in forward direction?

${\mathrm{I}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{l}\left(\mathrm{g}\right)\hspace{0.17em}\mathrm{Take} ∆\mathrm{H}°=+150 \mathrm{kJ}$

1. Increase in concentration of I

2. Increase in total pressure

3. Decrease in concentration of I₂

4. Increase in temperature

A reversible reaction is said to have attained equilibrium, when

1. Backward reaction stops

2. Both backward and forward reactions take place at equal speed

3. Both backward and forward reactions stop

4. Concentration of each of the reactants and products becomes equal

In what manner will increase of pressure affect the following equation?

$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

1. Shift in the reverse direction

2. Shift in the forward direction

3. Increase in the yield of hydrogen

4. No effect

The equilibrium between water and its vapour, in an open vessel

1. Can be achieved

2. Depends upon pressure

3. Cannot be achieved

4. Depends upon temperature

Which of the following equilibrium, in gaseous phase, would be unaffected by an increase in pressure?

1. ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$

2. ${\mathrm{N}}_2+{\mathrm{O}}_2\rightleftharpoons 2\mathrm{NO}$

3. ${\mathrm{N}}_2{\mathrm{O}}_4\rightleftharpoons 2{\mathrm{NO}}_2$

4. ${\mathrm{CO}}_2+\frac{1}{2}{\mathrm{O}}_2\rightleftharpoons {\mathrm{CO}}_2$

A saturated solution of non-radioactive sugar was taken and a little radioactive sugar was added to it. A small amount of it gets dissolved in solution and an equal amount of sugar was precipitated. This proves

1. The equilibrium has not been established in the solution

2. Radioactive sugar can displace non-radioactive sugar from its solution.

3. Equilibrium is dynamic in nature

4. None of the above

When two reactants A and B are mixed to give products C and D, the reaction quotient Q, at the initial stages of the reaction

1. is zero

2. decreases with time

3. is independent of time

4. increases with time