Solutions practice · Mixed difficulty

Which of the following solutions boils at the highest temperature

Which of the following on addition in 1.0 molal KI solution will give rise to increase a vapour pressure?

A solution has $80 \% \frac{\mathrm{w}}{\mathrm{w}} \mathrm{NaOH}$ with density $2 \text{g L}^{-1}.$ Find

(a) Molarity $\quad$ (b) Molality of solution

Assertion : One molal aqueous solution of urea contains $60 {~g}$ of urea in $1 {~kg}(1000 {~g})$ water.

Reason : Solution containing one mole of solute in $1000 {~g}$ solvent is called as one molal solution.

A solution is prepared by mixing $8.5 \mathrm{~g}_{\text {of }} \mathrm{CH}_2 \mathrm{Cl}_2$ and $11.95 \mathrm{~g}$ of $\mathrm{CHCl}_3$. If vapour pressure of $\mathrm{CH}_2 \mathrm{Cl}_2$ and $\mathrm{CHCl}_3$ at $298 \mathrm{~K}$ are 415 and $200 \mathrm{~mmHg}$ respectively, the mole fraction of $\mathrm{CHCl}_3$ in vapour form is :
(Molar mass of $\mathrm{Cl}=35.5 \mathrm{~g} \mathrm{~mol}^{-1}$ )

$11.2 \mathrm{~L}$ of ${HCl}({g})$ is completely dissolved in $500 \mathrm{~ml}$ of aqueous solution. The molality of the solution is

Dissolution of a solute is an exothermic process if :

What is the molality of pure water?

What volumes of $1 \mathrm{~M} \, \, \& \, \, 2 \mathrm{~M} \mathrm{~H}_2 \mathrm{SO}_4$ solution are required to produce $2 \mathrm{~L}$ of $1.75 \mathrm{~M~H}_2 \mathrm{SO}_4$ solution?

11.1 g of $CaCl_2$ is present in 100 ml of the aqueous solution. The chloride ion concentration is

In an osmotic pressure measurement experiment, a $5\%$ solution of compound ‘X’ is found to be isotonic with a $2\%$ acetic acid solution . The gram molecular mass of ‘X’ is

The normality of $2.3\;\mathrm{M}\;{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ solution is

The temperature at which $10 \%$ aqueous solution $(w / V)$ of glucose exhibits the osmotic pressure of $16.4 \mathrm{~atm}$, is $\left(R=0.082 \mathrm{~dm}^3 \mathrm{~atm} \mathrm{~K} \mathrm{~Kol}^{-1}\right)$

Statement I: Reverse osmosis is used in the desali- nation of sea water.

Statement II: When the applied pressure is more than the osmotic pressure, pure water is squeezed out of sea water through the membrane.

Equimolal solutions of A and B show depression in freezing point in the ratio $2 : 1.$ A remains in its normal state in solution. $B$ will be ……. in solution:

Statement - I: When an ideal binary solution of liquids A and B is distilled, the boiling point of
the distillate becomes lower than that of the parental liquid solution.

Statement - II: When an ideal binary solution of liquids A and B is distilled, the distillate
contains relatively larger amount of the more volatile liquid.

Which of the following statements is false?

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

The degree of dissociation $(\alpha)$ of a week electrolyte, $\mathrm{A}_2 \mathrm{SO}_4$ is related to Vant Hoff factor (i) by the expression

If molality of the dilute solutions is doubled, the value of molal depression constant $\left({K}_{{f}}\right)$ will be

A liquid solution is formed by mixing 10 moles of aniline and 20 moles of phenol at a temperature where the vapour pressures of pure liquid aniline and phenol are $90$ and $87 \mathrm{~mm} \mathrm{~Hg},$ respectively. The possible vapour pressure of solution at that temperature is

$1.2 \% \mathrm{NaCl}$ solution is isotonic with $7.2 \%$ glucose solution. What will be the van't Hoff factor ' $i$ ' for $\mathrm{NaCl}$ ?

Two liquids $A$ and $B$ are mixed in a ratio of $2: 3$. If $P_A^{\circ}=100 \,{mmHg}$ and $P_B^{\circ}=300 \,{mmHg}$, then the mole fraction of $A$ in vapour phase will be

Which method cannot be used to find out the molecular weight of non-volatile solute?

The boiling point of $0.2 \mathrm{~mol} \mathrm{~kg}^{-1}$ solution ${X}$ in water is greater than equimolal solution of ${Y}$ in water. Which one of the following statements is true in this case?

Two liquids X and Y form an ideal solution at 300K,vapour pressure of the solution containing 1 mol of X and 3, mol of Y is 550 mmHg. At the same temperature, if 1 mol of Y is further added to this solution, vapour pressure of the solution increases by 10 mmHg. Vapour pressure (in mmHg)of XandY in their pure states will be, respectively

Assertion: Soda bottles are sealed under high pressure.

Reason: High pressure increases the solubility of carbon dioxide gas.

The relationship which describes the variation of vapour pressure of a liquid with temperature is called :

The value of Henry's constant $K_{\mathrm{H}}$ is

Which solution will have least vapour pressure?