Relative Lowering of Vapour Pressure

A saturated solution of $\mathrm{Mg}(\mathrm{OH}{)}_2$ has a vapor pressure of $759.5 \mathrm{mm} \mathrm{of} \mathrm{Hg} \mathrm{at} 373 \mathrm{K}$. Calculate solubility and ${\mathrm{K}}_{\mathrm{sp}} \mathrm{of} \mathrm{Mg}(\mathrm{OH}{)}_2$. (Assume $\mathrm{m}=\mathrm{M}$)

Which of the following can be measured by the Ostwald-Walker method?

The lowering of vapour pressure in a saturated aq. solution of salt $\mathrm{A} \mathrm{B}$ is found to be $0.108$ torr. If vapour pressure of pure solvent at the same temperatuare is $300$ torr, find the solubility product of salt $\mathrm{AB}$:

The vapour pressure of an aqueous solution of cane sugar (molar weight=$342$) is $756 \mathrm{mm}$ at $100°\mathrm{C}$. How many grams of sugar are present per $1000 \mathrm{g}$ of water? Report the answer in the nearest integer

What is the vapour pressure of a solution containing $15.6 \mathrm{g}$ of water and $1.68 \mathrm{g}$ of sucrose $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$ at $100° \mathrm{C}$?

Give your answer by rounding off to the nearest integer value.Molecular weight of sucrose is $342$.

The pressure of the water vapour of a solution containing a non-volatile solute is $2\%$ below that of the vapour of pure water. Determine the molality of the solution.

Round off your answer to nearest integer value.

An aqueous solution of $2\%$ non-volatile solute exerts a pressure of $1.004$ bar at the normal boiling point of the solvent. What is the molar mass of the solute? (Write the answer without units)

Two beaker are placed in a sealed flask. Beaker A initially contained 0.15 mol of naphthalene (non-volatile) in 117 g of benzene and beaker B initially contained 31 g of an unknown compound (non-volatile, non-electrolytic) in 117 g of benzene. At equilibrium, beaker A is found to have lost 7.8 g of weight. Assume ideal behaviour of both solutions to answer the following question.

The molar mass of solute in solution B is closest to:

In an experiment, $18.04 \mathrm{g}$ of mannitol were dissolved in $100 \mathrm{g}$ of water. The vapour pressure of water was lowered by $0.309 \mathrm{mm} \mathrm{Hg}$ from $17.535 \mathrm{mm} \mathrm{Hg}$. Calculate the molar mass of mannitol.

The vapour pressure of water at $20°\mathrm{C}$ is $17 \mathrm{mm} \mathrm{Hg}$. Calculate the vapour pressure of a solution containing $2.8 \mathrm{g}$ of urea $\left({\mathrm{NH}}_2{\mathrm{CONH}}_2\right)$ in $50 \mathrm{g}$ of water. $\left(\mathrm{N}=14,\mathrm{C}=12,\mathrm{O}=16,\mathrm{H}=1\right)$

The vapour pressure of $2.1\%$ solution of a non-electrolyte in water at $100°\mathrm{C}$ is $755 \mathrm{mm} \mathrm{Hg}$. Calculate the molar mass of the solute.

Relative vapour pressure lowering depends only on.

Vapour pressure of solution of a non volatile solute is always

Lowering of the vapour pressure of the solution:

Derive the relationship between relative lowering of vapour pressure and molar mass of solute.

What is lowering of vapour pressure of a solution?

Find the value of mole fraction of the solute when vapour pressure of glucose is $750 \mathrm{mm} \mathrm{Hg}$ at $373 \mathrm{K}$ in dilute solution.

Find the correct relation between ${\mathrm{pK}}_{\mathrm{a}1} \mathrm{and} {\mathrm{pK}}_{\mathrm{a}2}$ of acids HA₁ and HA₂ (assuming they are taken in same concentration), if lowering of vapour pressure $\Delta \mathrm{P}_{1}$ of an aqueous solution of acid HA₁ and $\Delta \mathrm{P}_{2}$ of an aqueous solution of acid HA₂, are related as $∆{\mathrm{P}}_1>∆{\mathrm{P}}_2$.
 

An ideal solution of two pure liquids $\mathrm{A}$ and $\mathrm{B}$ are having the vapour pressure of $100$ and $400 \mathrm{torr}$ respectively at the temperature $\mathrm{T}$. The liquid solution of $\mathrm{A}$ and $\mathrm{B}$ is made up of $1 \mathrm{mole}$ of each $\mathrm{A}$ and $\mathrm{B}$. Then, find the pressure when $1 \mathrm{mole}$ of mixture has been vaporised.

The relative lowering of the vapour pressure of an aqueous solution containing a non-volatile solute is $0.0125$. What is the molality of the solution?