Solutions practice · Mixed difficulty

Two liquids $\mathrm{A}$ and $\mathrm{B}$, form an ideal solution. At a specific temperature, the vapour pressure of pure ' $\mathrm{A}$ ' is $200 \mathrm{~mm}$ of ${Hg}$. While that of pure $\mathrm{B}$ is $100 \mathrm{~mm}$ of ${Hg}$. The vapour over mixture consists of $50 \%$ moles of $\mathrm{A}$, what is the $\%$ of $\mathrm{A}$ in the liquid ?

The freezing point depression of 0.1 molal solution of acetic acid in benzene is $0.256 \mathrm{~K} . k_f$ for benzene is $5.12 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. What conclusion can you draw about the molecular state of acetic acid in benzene?

Maximum lowering of vapour pressure is observed in the case of

The vapour pressure of two liquids $P$ and $Q$ are 80 and 60 torr resp. The total vapour pressure of solution obtained by mixing 3 mole of $P$ and 2 mol of $Q$ would be

At $300 \mathrm{~K} \,36 \mathrm{~g}$ of glucose present in a litre of its solution has an osmotic pressure of $4.98 \,\mathrm{bar}$. If the osmotic pressure of the solution is 1.52 bar at the same temperature, what would be its concentration?

Essential quantity of ammonium sulphate taken for preparation of 1 molar solution in 2 litres is

When $100\, {ml}$ of $\frac{{M}}{10} {H}_2 {SO}_4$ is mixed with $500 \,{ml}$ of $\frac{{M}}{10} {NaOH}$ then nature of resulting solution and normality of excess of reactant left is

Calculate the entropy change for vaporisation of water if latent heat of vaporisation for water is $540 {cal} / {g}$. Given $K_b$ for ${H}_2 {O}=0.51 {~K} /$ molality.

Which of the aqueous equimolal solution will have its vapour pressure near to solvent?

The solubility of a specific non-volatile salt is $4 \mathrm{~g}$ in $100 \mathrm{~g}$ of water at $25^{\circ} \mathrm{C}$. If $2.0 \mathrm{~g}, 4.0 \mathrm{~g}$ and $6.0 \mathrm{~g}$ of the salt added of $100 \mathrm{~g}$ of water at $25^{\circ} \mathrm{C}$, in system $X, Y$ and $Z$. The vapour pressure would be in the order: