Solutions practice · Mixed difficulty

A certain substance ‘A’ tetramerises in water to the extent of 80%. A solution of 2.5 g of A in 100 g of water lowers the freezing point by $0.3^\circ C$. The molar mass of A is

Osmotic pressure present in the fluid inside the blood cell is equivalent to

Mixture of $1 \mathrm{~mol}$ benzene $(p_{\text {benzene}}^{\circ}=42 \mathrm{~mm})$ and $2 \mathrm{~mol}$ toluene $\left(p_{\text {toluene}}^\circ=36 \mathrm{~mm}\right)$ will have

Dry air was passed successively through a solution of $5 \mathrm{~g}$ of a solute in $180 \mathrm{~g}$ of water and then through pure water. The loss in weight of solution was $2.50 \mathrm{~g}$ and that of pure solvent is $0.04 \mathrm{~g}.$ The molecular weight of the solute is

Which of the following behaviour is true about the ideal binary liquid solution of liquids '${A}$' and '${B}$', if $P_{{A}}^{\circ} < P_{{B}}^{\circ}?$

Which of the following is incorrect?

The vapour pressure of water is 12.3 kPa at 300 K.
What is the vapour pressure of 1 molal aqueous
solution of a non- volatile solute at 300 K?

The density $\left( {i\mathrm{n}\;\mathrm{ g}\;\mathrm{m}\;{\mathrm{L}^{ - 1}}} \right)$ of a ${3.60\;M}$ sulphuric acid solution that is $29\;\% \;{H_2}S{O_4}\left( {\mathrm{molar}\;\mathrm{ mass} = 98\;\mathrm{g}\;\mathrm{mo}{\mathrm{l}^{ - 1}}} \right)$ by mass will be

For an ideal solution of ${A}$ and ${B}, Y_{{A}}$ is the mole fraction of ${A}$ in the vapour phase at equilibrium. Which of the following plot should be linear?

Assertion: $0.1 \mathrm{~M}$ solution of $\mathrm{NaCl}$ have low freezing point than $0.1 \mathrm{~M}$ urea solution.

Reason: Van't Hoff factor (No. of particles) for $\mathrm{NaCl}$ is more than urea.

When attraction between $A - B$ is more than that of $A - A$ and $B - B$, the solution will show…..deviation from Raoult’s law

Cyclohexane and ethanol at a particular temperature have vapour pressure of $280 {~mm}$ and $168 {~mm}$ respectively. If these two solutions having mole fraction value of cyclohexane equal to 0.32 are mixed and the mixture has a total vapour pressure of $376 {~mm}$, will the mixture be an ideal solution?

A solution of $1.25 \mathrm{~g}$ of $P$ in $50 \mathrm{~g}$ of water lowers the freezing point of water by $0.3^{\circ} \mathrm{C}$. Molar mass of $P$ is 94. $K_{f(\text { water })}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. The degree of association of $P$ in water is

The total vapour pressure of a 4 mole $\%$ solution of $\mathrm{NH}_3$ in water at $293 \mathrm{~K}$ is 50.0 torr. The vapour pressure of pure water is 17.0 torr at this temperature. Applying Henry's and Raoult's laws, the total vapour pressure for a 5 mole $\%$ solution is

Sodium sulphate is soluble in water, while barium sulphate is sparingly soluble because :

The vapour pressure of water at $20^\circ C$ is ${17.54\;\mathrm{mm}}$. When 20 g of a non-ionic, substance is dissolved in ${100\;g}$ of water, the vapour pressure is lowered by ${0.30\;\mathrm{mm}}$. What is the molecular mass of the substance?

When a saturated solution of sodium chloride is heated, it:

Assertion (A): When methyl alcohol is added to water, boiling point of water increases.

Reason ( R ): When a volatile solute is added to a volatile solvent, elevation in boiling point is observed.

Statement II: The vapour pressure of $0.1 \mathrm{~M}$ sugar solution is more than that of $0.1 \mathrm{~M} \mathrm{~KCl}$ solution.

Statement II: Lowering of vapour pressure is directly proportional to the number of species present in the solution.

A sugar syrup weighing $214.2 \mathrm{~g}$, contains $34.2 \mathrm{~g}$ of water. The molal concentration is:

Consider following solutions in given solvents:
I: $0.3 \mathrm{~M}$ aqueous glucose solution
II: $0.2 \mathrm{~M}$ aqueous sodium chloride solution
III: $0.3 \mathrm{~M}$ aqueous ammonium phosphate solution
IV: $0.4 \mathrm{~M}$ benzoic acid in benzene (dimerises upto $50 \%$)
Select incorrect statement from given options for the above given solutions:

At $27^\circ C$, the osmotic pressure of a solution containing 4.0 g solute (molar mass = 246) per litre at $27^\circ C$ is :$(R = 0.0821\;\mathrm{atms}.\mathrm{mo}{\mathrm{l}^{ - 1}}\;K)$

Assertion : If a liquid solutemore volatile than the solvent is added to the solvent, the vapour pressure of the solution may increase i.e., $p_{{s}}>p^0$.

Reason : In the presence of a more volatile liquid solute, only the solute will form the vapours and solvent will not.

Liquid $M$ and liquid $N$ form an ideal solution. The vapour pressures of pure liquids $M$ and $N$ are 450 and 700 mmHg, respectively, at the same temperature. Then correct statement is
${x_M} =$ mole fraction of $M$ in solution; $\,\,\,\,\,\,\,\,\,\,\,{x_N} =$ mole fraction of $N$ in solution;
${y_M} =$ mole fraction of $M$ in vapour phase; $\,\,\,\,\,\,\,\,\,\,\,\,\,\,{y_N} =$ mole fraction of $N$ in vapour phase;

Which should exhibit abnormal osmotic pressure

Assertion: The activity coefficients of the components in an ideal solution are equal to 1.

Reason: In an ideal solution, the interactions between the two components are the same as the interactions between like molecules.

Which of the following pairs of solutions can be expected to be isotonic at the same temperature

$58.5 \mathrm{~g}$ of $\mathrm{NaCl}$ and $180 \mathrm{~g}$ of glucose were separately dissolved in $1000 \mathrm{~mL}$ of water. Identify the correct statement regarding the elevation of boiling point (bp) of the resulting solution.

Calculate the mass of a non-volatile solute (molar mass 40), which should be dissolved in $114{~g}$ octane to reduce its vapour pressure to $80 \%$.

$20\;g$ of binary electrolyte (mol. wt. =100) are dissolved in $500\;g$ of water. The depression in freezing point of the solution is $0.74^\circ C\;({k_f} = 1.86\;K{m^{ - 1}})$ the degree of ionisation of the electrolyte is