Solutions practice · Medium

The ratio of elevation in boiling point for ${Fe}_3\left[{Fe}({CN})_6\right]_2$ (assume complete ionization) to elevation in boiling point of sugar solution of equal molal concentration is

Statement I: Vapour pressure of water is less than 1.013 bar at $373 \mathrm{~K}$.

Statement II: Water boils at $373 \mathrm{~K}$ as the vapour pressure of water at this temperature becomes equal to atmospheric pressure

Assertion (A): 0.1 M solution of glucose has higher increment in the freezing point than 0.1 M solution of urea.

Reason (R): $\mathrm{K}_{\mathrm{f}}$ for both has different values.

Find out molality of $0.8 \mathrm{~M} \mathrm{~H}_2 \mathrm{SO}_4$ solution having density of solution equal to $1.02 \mathrm{~gm} / \mathrm{ml}$ (Nearest integer)

Assertion (A) : At low concentration, benzene and toluene forms ideal solution.

Reason (R) : Components with structural similarity forms ideal solution

Ice begins to separate at $-0.744^{\circ} \mathrm{C}$ from an aqueous solution containing $2.4 \mathrm{~g}$ of a non-volatile, non-electrolyte in $100 \mathrm{~g}$ water. The osmotic pressure of the solution at $27^{\circ} \mathrm{C}$ is $\left(K_{\mathrm{f}}\right.$ for water $=1.86,$ assume molality $=$ molarity)

Statement I: The freezing point of water is depressed by the addition of glucose.

Statement II: Entropy of solution is less than entropy of pure solvent.

Consider following terms $(\mathrm{m}=$ molality $)$ :

I : ${mK}_{{b}};\quad$ II: ${mK}_{{b}} {i}\quad$ III : $\frac{\Delta {T}_{{b}}}{{i}}\quad$ IV : $K_b$

Terms which can be expressed in degree (temperature) are

The degree of dissociation ($\propto$) of a weak electrolyte, ${A_x}By$ is related to vant Hoff factor (i) by the expression

50 g of an acid is dissolved in one litre aqueous solution. Distribution coefficient in favour of ether is 3. Acid left in aqueous layer when solution is shaken with one litre ether :

The solution from the following with highest depression in freezing point/lowest freezing point is

Select correct statement(s) :

$0.1435 \mathrm{~m}$ solution of a non-volatile, non-electrolyte solute has the freezing point 0.73 degrees lower than that of benzene. What is the value of molal freezing point depression constant of benzene?

The plots of $\frac{1}{{{X_A}}}\;vs.\;\frac{1}{{{Y_A}}}$ (where ${X_A}\;\mathrm{and}\;{Y_A}$ are the mole fraction of liquid A in liquid and vapour phase respectively) is linear with slope and intercepts respectively:

One gram of silver gets distributed between $10{\kern 1pt} \,\mathrm{c}{\mathrm{m}^3}$ of molten zinc and $100\,\mathrm{c}{\mathrm{m}^3}$ of molten lead at $8000^\circ C.$ The percentage of silver still left in the lead layer in approximately

18 g of Glucose is added to 178.2 g of water the vapour pressure of water for this aqeous solution at $100^\circ C$ is.

Assertion (A): Sum of mole fraction of all components in a mixture is 1.

Reason (R): Mole fraction is temperature dependent mode of concentration.

The osmatic pressure of a 5% (wt./vol) solution of cane sugar at $150^\circ C$ is

Assertion (A) : The pressure exerted by a liquid in equilibrium with its liquid at a given temperature is called its vapour pressure.

Reason (R) : If a non-volatile solute is added to a solvent to give a solution, the vapour pressure of the solution is found to be greater than the vapour pressure of the pure solvent.

Which of the following is incorrect regarding solution showing negative deviation from Raoult's law?

The increase in boiling point of a solution containing 0.6 g urea in 200 g water is $0.50^\circ \mathrm{C}$ .Find the molal elevation constant.

What is the molality of a solution which contains $18 {~g}$ of glucose $\left({C}_6 {H}_{12} {O}_6\right)$ in $250 {~g}$ of water

Boiling point of chloroform was raised by $0.323 \mathrm{~K}$, when $0.5143 \mathrm{~g}$ of anthracence was dissolved in its $35 \mathrm{~g}$. Molecular mass of anthracence is $\left({K}_{{b}}\right.$ for $\left.{CHCl}_3=3.9 \, \mathrm{k}-\mathrm{kg}-\mathrm{mol}^{-1}\right)$

An ideal solution was found to have a vapour pressure of 80 torr when the mole fraction of a non-volatile solute was $0.2.$ What would be the vapour pressure of the pure solvent at the same temperature?

The solution containing 4.0 g of PVC in 1 L of
dioxane was found to have osmotic pressure of
0.006 atm at 300 K. The molecular mass of the
polymer PVC is

$1.0 \mathrm{~g}$ of a mono basic acid $\mathrm{HA}$ in $100 \mathrm{~gm}$ water lowers the freezing point by $0.155 \mathrm{~K}$. If 0.75 gm of same acid requires $25 \mathrm{ml}$ of $\mathrm{N} / 5 \mathrm{NaOH}$ solution for complete neutralization then % degree of ionization of acid is $\left(K_f\left(H_2 \mathrm{O}\right)=1.86 \mathrm{~kg} \mathrm{~mol}^{-1}\right)$

Which pair will not be isotonic

What will be the molarity of a $200 \mathrm{~mL}$ solution containing $1.2 \mathrm{~g}$ of urea?

If $0.1 \mathrm{~M}$ solution of ${NaCl}$ has same osmotic pressure as $0.1 \mathrm{~M}$ solution of ${CaCl}_2,$ then the degree of dissociation of ${CaCl}_2$ will be

The amount of solute (molar mass $60 \mathrm{~g} \mathrm{~mol}^{-1}$) that must be added to $180 \mathrm{~g}$ of water so that the vapour pressure of water is lowered by $10 \%$ is