Solutions practice · Easy

The osmotic pressure of a non-volatile solute in $\mathrm{C}_6 {H}_6$ at $25^{\circ} {C}$ is $20.66 {Nm}^{-2}$. If the solution had a concentration of $2 {~g} / {dm}^3$, what is molar mass of solute?

5 L of a solution contains 25 mg of $CaC{O_3}.$ What is its concentration in ppm? (mol. wt. of $CaC{O_3}$ is 100)

When ${Hgl}_2$ is added to an aqueous solution of ${Kl}$

During depression of freezing point in a solution the following are in equilibrium

ASSERTION : Molar heat of vaporisation of water is greater than benzene.

REASON : Molar heat of vaporisation is the amount of heat required to vaporise one mole of liquid at constant temperature.

The ratio of vapour pressure over solution phase on mixing two immiscible liquids is equal to :

According to phase rule, if $P = 3,C = 1,$ then F must be equal to :

Aqueous solutions of two acids having same concentrations of common ion $\left[ {{\mathrm{H}^ + }} \right]$ are called:

A liquid is in equilibrium with its vapours at its boiling point. On the average the molecules in the two phases have equal :

The amalgam of mercury in sodium is an example of

The reverse of fusion is freezing and it is :

Select the incorrect statement :

Which of the following has minimum freezing point?

The vapour pressure $(VP)$ of a dilute solution of non-volatile solute is $P$ and the $VP$ of pure solvent is ${P_0}$, the lowering of the $VP$ is :

A thermometer which can be used only for accurate measurement of small differences in temperature is known as a:

An aqueous solution is 1.0 molal in KI. Which change will cause the vapour pressure of solution to increase :

A solute is soluble in two immiscible liquids which are present in a mixture. The concentration of the solute in the upper layer will be :

Which has the minimum freezing point?

The solubility of a solid in a liquid depends on :

A dry air is passed through the solution, containing the $10 \mathrm{~g}$ of solute and $90 \mathrm{~g}$ of water and then it is passed through pure water. There is the depression in weight of solution by $2.5 \mathrm{~g}$ and in weight of pure solution by $0.05 \mathrm{~g}$. Calculate the molecular weight of solute.

Assertion (A): Isotonic solutions must have same elevation in boiling point.

Reason (R): Osmotic pressure, $\pi=i C R T$

The vapour pressure of water at room temperature is lowered by $5 \%$ on dissolving a non-volatile solute in it. The molality of the solution is

Maximum freezing point will be for 1 molal solution, assuming equal ionization in each case:

Which of the following is correct for a solution showing positive deviations from Raoult's law?

Van’t Hoff factor more than unity indicates that the solute in solution has

What is the total number of moles of ${H_2}S{O_4}$ needed to prepare $5.0\;L$ of a $2.0\;M$ solution of ${H_2}S{O_4}$ ?

Maximum lowering of vapour pressure is observed in the case of

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: