Solutions practice · Easy

Option A ($0.0789,4.76$) is correct because it correctly calculates the mole fraction and molality of the solute using Raoult's Law.

Option A (Moist air) is correct because it represents a solution where liquid (water) is dispersed in a gas (air).

The correct answer is 50000 because isotonic solutions have the same molar concentration, allowing us to equate the concentrations and solve for the protein's molecular mass.

Option D (Neither $\mathrm{H}_2 \mathrm{O}$ nor $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$ in their pure state) is correct because azeotropes boil at a constant temperature and cannot be separated by simple distillation.

Option D (All of the above) is correct because adding salt to snow lowers the freezing point of water, causing the ice to melt at the ambient temperature.

Option B (glucose) is correct because the calculated molar mass of the unknown substance X is approximately 174 g/mol, which is close to the molar mass of glucose.

The correct answer is A because the statement describes colligative properties, specifically the effect of solutes on freezing and boiling points.

The correct answer is B (Same as what would be if the glass plate were removed) because vapor pressure depends only on temperature and the nature of the liquid, not the presence of a glass plate.

Option A (Raoult) is correct because Raoult's Law states that the relative lowering of vapor pressure is equal to the mole fraction of the non-volatile solute.

Option C (Mole fraction of solute) is correct because Raoult's law states that the relative lowering of vapor pressure is equal to the mole fraction of the solute in the solution.

Option B (Plot of $P_{\text {total}}$ vs $X_{{B}}$ is linear with +ve slope) is correct because the total pressure is a linear function of the mole fraction of B with a positive slope when $P_{{A}}^{\circ} < P_{{B}}^{\circ}$.

Option B (Negative) is correct because stronger A-B interactions compared to A-A and B-B lead to lower vapor pressure and negative deviation from Raoult's law.

Option A (The hydration energy of sodium sulphate is more than its lattice energy) is correct because the solubility of an ionic compound depends on the balance between hydration energy and lattice energy.

Option B (Becomes unsaturated) is correct because the solubility of most salts, including NaCl, increases with temperature, allowing more solute to dissolve.

Option B (0.4 atm) is correct because the osmotic pressure is calculated using the formula $\pi = \frac{n}{V}RT$, where n is the number of moles of solute, V is the volume in liters, R is the gas constant, and T is the temperature in Kelvin.

Option B (Aqueous solution of common salt) is correct because common salt (NaCl) dissociates into ions in solution, leading to an increase in the number of particles and thus abnormal osmotic pressure.

The correct answer is 0.1 M $Ca(NO_3)_2$ and 0.1 M $Na_2SO_4$ because they have the same van't Hoff factor (i) and concentration, leading to the same osmotic pressure.

Option A (10) is correct because it is the mass of the non-volatile solute calculated using Raoult's law.

Option B is correct because Raoult's law for dilute solutions states that the relative lowering of vapor pressure is equal to the mole fraction of the solute.

Option A is correct because a hypotonic solution has a lower osmotic pressure compared to another solution.

Option A (0.1 M) is correct because the molarity is half of the normality for Na2CO3, since it's a dipositive salt.

Option C (1.176 atm) is correct because the partial pressure of dry air is the total pressure minus the partial pressure of water vapor, calculated using mole fraction.

Option A (0.0018) is correct because it accurately calculates the relative lowering in vapor pressure using the isotonic condition and Raoult's law.

Option A (0.51) is correct because it represents the ebullioscopic constant ($K_b$) calculated using the elevation in boiling point and the molality of the glucose solution.

The correct answer is A ($0.1\;\mathrm{M }\;\mathrm{BaC}{\mathrm{l}_2}$) because it has the highest van't Hoff factor, leading to the greatest lowering of vapor pressure.

Option C ($i = \frac{{\mathrm{normal}\;\mathrm{ molecular}\;\mathrm{ mass}}}{{\mathrm{observed }\;\mathrm{molecular}\;\mathrm{ mass}}}$) is correct because the van't Hoff factor is defined as the ratio of normal molecular mass to observed molecular mass.

Option A (Statement I and statement II both are correct) is correct because Raoult's law is indeed applicable for dilute solutions only, and Henry's law applies to the solution of gas in liquid.

The correct answer is B ($2.46 {~atm}$) because it correctly applies the osmotic pressure formula using the given concentration, gas constant, and temperature.

Option C (Raoult's law) is correct because Raoult's law states that the relative lowering of vapor pressure of a solution containing a non-volatile solute is directly proportional to the mole fraction of the solute.

Option D ($100.156^{\circ} {C}$) is correct because it involves calculating the elevation in boiling point using colligative properties and van't Hoff factors for NaCl and BaCl2.