Embibe Experts Solutions for Chapter: Solutions, Exercise 3: Exercise-3

$1.22 \mathrm{g}$ of Benzoic acid is dissolved in $100 \mathrm{g}$ of Acetone and $100 \mathrm{g}$ of Benzene separately. Boiling point of the solution in Acetone increases by $0.17°\mathrm{C},$ while that of, in the Benzene increases by $0.13°\mathrm{C}; {\mathrm{K}}_{\mathrm{b}}$ for Acetone and Benzene are $1.7 \mathrm{K} \mathrm{kg}{ \mathrm{mol}}^{-1}$ and $2.6 \mathrm{K} \mathrm{kg}{ \mathrm{mol}}^{-1}$respectively. Molecular weight of Benzoic acid in Benzene is $\mathrm{X}$ and in Acetone is $\mathrm{Y}$. Calculate $\mathrm{X}+\mathrm{Y}$?

The elevation in boiling point of a solution of $13.44 \mathrm{g}$ of ${\mathrm{CuCl}}_2$ in $1 \mathrm{kg}$ of water using the following information, will be (Molecular weight of ${\mathrm{CuCl}}_2=134.4$ and ${\mathrm{K}}_{\mathrm{b}}=0.52 \mathrm{K} {\mathrm{molal}}^{-1}$) : (Report the answer in two decimal places)

For a dilute solution containing $2.5 \mathrm{g}.$of a non- electrolyte solute. in $100 \mathrm{g}$ of water, the elevation in boiling point at $1$ atm pressure pressure is $2°\mathrm{C}.$ Assuming concentration of  solute is much lower than the concentration of solvent, the vapour pressure $(\mathrm{mm}$ of $\mathrm{Hg}$ )  of the solution is (take ${\mathrm{K}}_{\mathrm{b}}=0.76 \mathrm{K} \mathrm{kg}$ ${\mathrm{mol}}^{-1} )$

Benzene and naphthalene form an ideal solution at room temperature. For this process, the true statement(s) is (are):

${\mathrm{MX}}_2$ dissociates into ${\mathrm{M}}^{2+}$ and ${\mathrm{X}}^{-}$ ions in an  aqueous solution, with a' degree of dissociation $\left(\mathrm{\alpha }\right)$ of $0.5.$  The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is 

Mixture(s) showing positive deviation from Raout's law at ${35}^{\mathrm{o}}\mathrm{C}$ is (are)

For a solution formed by mixing liquids $\mathrm{L}$ and $\mathrm{M},$ the vapour  pressure of $\mathrm{L}$ plotted against the mole  fraction of $\mathrm{M}$ in solution is shown in the following figure. Here ${\mathrm{x}}_{\mathrm{L}}$ and ${\mathrm{x}}_{\mathrm{M}}$ represent mole fractions of $\mathrm{L}$  and $\mathrm{M},$ respectively, in the solution. The correct statement(s) applicable to this system is (are):

The plot given below shows $\mathrm{P}-\mathrm{T}$ curves (where $\mathrm{P}$ is the pressure and $\mathrm{T}$ is the temperature) for two solvents $\mathrm{X}$ and $\mathrm{Y}$ and isomolal solutions of $\mathrm{NaCl}$ in these solvents. $\mathrm{NaCl}$ completely dissociates in both the solvents.

On addition of equal number of moles of a non-volatile solute $\mathrm{S}$ in equal amount (in $\mathrm{kg}$ ) of these solvents, the elevation of boiling point of solvent $\mathrm{X}$ is three times that of solvent $\mathrm{Y}.$ Solute $\mathrm{S}$ is known to undergo dimerization in these solvents. If the degree of dimerization is $0.7$ in solvent $\mathrm{Y},$ the degree of dimerization in solvent $\mathrm{X}$ is: