Gases in Liquids

Q. Select the correct order of solubility for the following gases in aqueous solution:

1. $HCl>O_2>N{H}_3$
2. $N{H}_3>HCl>O_2$
3. $HCl>N{H}_3>O_2$
4. $O_2>HCl>N{H}_3$

Q. Step-I: 0.5 L of saturated $Mg(OH{)}_2$ (aq.) is in contact with $Mg(OH{)}_2$(s).
Step-II: 0.5 L of $H_{2}O$ is added to 0.5 L of solution in step (I) and the solution is vigorously stirred, undissolved $Mg(OH{)}_2$(s) remains.
Step-III: 100 mL of the clear solution in step (II) is removed and added to 0.5 L of 0.1 M $HCl$(aq.).
Step-IV: 25 mL of the clear solution in step (II) is removed and added to 225 mL of 0.06 M $MgC{l}_2$(aq.) $(K_{sp},Mg(OH{)}_2=3.2\times {10}^{-11})$.
Which of the following are correct choices about above steps?

1. $\text{Concentration of}M{g}^{2+}\text{(aq.) in step (II) is}2\times {10}^{-4}M$
2. $\text{Concentration of}M{g}^{2+}\text{(aq.) in step (III) is}3.33\times {10}^{-5}M$
3. $\text{Concentration of}M{g}^{2+}\text{(aq.) in step (IV) is nearly equal to}0.054M$
4. $\text{Precipitation of}Mg\left(OH{)}_2\right(s)\text{will occurs in step (III)}$

Q. For an exothermic dissolution process, increase in temperature will result in:

1. Cannot be predicted
2. Decrease in solubility
3. No change in solubility
4. Increase in solubility

Q. The order of solubility of oxygen in water is

1. Hot water > cold water
2. Cold water > hot water
3. Soluble equally in both
4. Cannot be predicted

Q. An exothermic process goes from state A to state B. If the temperature of the process is increased, the process moves towards

1. From state A to state B
2. From state B to state A
3. No heat flow occurs
4. Both will be in thermal equilibrium