Solutions practice · Mixed difficulty

Option A (Both A & R are true, R is the correct explanation of A) is correct because azeotropic solutions with lower boiling points exhibit positive deviations from ideal behavior.

Option A (3.2) is correct because the molality is calculated using the mole fraction of the solute and the molar mass of benzene.

Option C ($\mathrm{Al}_2(\mathrm{SO}_4)_3$) is correct because it has a van't Hoff factor (i=5) closest to that of $\mathrm{K}_4[\mathrm{Fe}(\mathrm{CN})_6]$ (i=5), resulting in similar osmotic pressure.

Option C (133.33) is correct because it is the molar mass calculated using the relative lowering of vapor pressure formula.

Option A ($20 \mathrm{~ml}$) is correct because using the dilution formula $M_1V_1 = M_2V_2$, we find that 20 ml of 0.5 M Urea is required to prepare 100 ml of 0.1 M Urea solution.

The correct answer is D (Liquid-gas, liquid-liquid and liquid-solid phases) because the distribution law applies to the distribution of a dissolved substance between any heterogeneous system.

Option D is correct because the freezing point depression depends on the solvent's cryoscopic constant, which varies between different solvents.

Option C is correct because Statement I is correct, but Statement II is false because the number of particles increases upon dissolution.

Option D ($D<B>A<C$) is correct because elevation in boiling point and depression in freezing point are colligative properties, and the order of freezing points is inverse to the order of boiling points.

Option A (+6) is correct because the oxidation number of Cr in CrO5 is determined considering the presence of peroxide linkages.

Option C (4/9) is correct because it correctly applies Raoult's Law and Dalton's Law to determine the mole fraction of A in the vapor phase.

Option A (348.8 g mol⁻¹) is correct because the molecular weight of the organic solute is calculated using the isotonic condition and the molar mass of urea.

Option A ($374.1128 \mathrm{~K}$) is correct because it is calculated by determining the molality, van't Hoff factor, and boiling point elevation, then adding the elevation to the normal boiling point of water.

Option A (Molefraction of solute) is correct because the relative lowering of vapor pressure is equal to the mole fraction of the solute according to Raoult's Law.

Option A ($34.2 \% \text{(w/w)}$ Sugar) is correct because the sugar solution has the highest molality, leading to the greatest boiling point elevation.

Option D (0.1) is correct because it is calculated by finding the mole fraction of water in the ideal solution.

Option C (3) is correct because, using the distribution coefficient formula, the percentage of silver left in the lead layer is approximately 3%.

The correct answer is A. $CaCl_2$ lowers the freezing point of water, preventing ice formation and minimizing road damage.

The correct answer is B (4) because the molality is calculated by dividing the moles of Na+ ions by the mass of water in kg.

Option B is correct because colligative properties depend only on the number of solute particles in a solution, not their nature.

Option C (428 mL and 572 mL) is correct because it satisfies the equation M1V1 + M2V2 = M_final * V_final, resulting in the correct final molarity.

Option A (Plasmolysis) is correct because plasmolysis is the process where cells shrink due to water loss when placed in a hypertonic solution.

Option C (Plant cell) is correct because plant cells have semipermeable membranes.

Option C ($101.04^\circ C$) is correct because the boiling point elevation is calculated using the van't Hoff factor (i=2 for KCl) and the molal elevation constant.

Option D (If Statement I is false but Statement II is correct) is correct because a solution, by definition, is a homogeneous mixture, meaning its composition is uniform throughout.

Option A (is higher than that of the dilute solution) is correct because osmotic pressure is directly proportional to the concentration of the solution.

Option A is correct because the molar mass calculated from the freezing point depression matches that of $Hg_2Cl_2$.

Option B (Glycol) is correct because glycol is commonly used as an antifreeze in automobile radiators due to its colligative properties.

Option B (If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1) is correct because osmotic pressure is a colligative property, and it develops due to osmosis, but the latter doesn't explain the former.

The correct answer is A because both statements are correct, and Statement II correctly explains why the vapor pressure of the sugar solution is higher than that of the KCl solution due to the number of solute particles.