Solutions practice · Easy

Option D (Lowering in freezing point) is correct because ethylene glycol acts as an antifreeze, lowering the freezing point of water.

Option B (1 M) is correct because the molarity is calculated by dividing the number of moles of glucose by the volume of the solution in liters.

Option A ($2/3$) is correct because it is calculated using Raoult's Law, which relates the vapor pressure of the solution to the mole fraction of the solvent.

Option C (Acetone and chloroform) is correct because they form hydrogen bonds, leading to stronger intermolecular forces and a decrease in vapor pressure.

Option D (All of these) is correct because the solubility of a gas in water is affected by the nature of the gas, temperature, and pressure of the gas.

The correct answer is that the mango loses water due to osmosis. Osmosis is the movement of water from a region of high water concentration (inside the mango) to a region of low water concentration (the concentrated salt solution).

Option A (The relative lowering of vapour pressure is equal to mole fraction of solute) is correct because that is the definition of Raoult's law for dilute solutions.

Option C (Zero) is correct because, according to the phase rule, F = C - P + 2, and substituting P = 3 and C = 1 gives F = 1 - 3 + 2 = 0.

Option A ($0.1\,M$) is correct because it is calculated using the osmotic pressure formula.

Option A (Ethanol + Acetone) is correct because the interaction between ethanol and acetone is weaker than the hydrogen bonding in pure ethanol, leading to positive deviation.

Option C (1) is correct because one mole of any ideal gas occupies 22.4 L at standard temperature and pressure (STP).

Option B ($1 \;N$) is correct because after dilution, the normality is calculated using the formula $N_1V_1 = N_2V_2$.

Option C (osmotic pressure) is correct because isotonic solutions, by definition, have the same osmotic pressure at a given temperature.

Option D (0.1) is correct because molarity is calculated by dividing normality by the basicity of the acid.

Option A (0.1) is correct because the mole fraction of HCl is calculated by dividing the moles of HCl by the total moles of the solution (HCl + water).

The correct answer is B (shows positive deviation from Raoult’s law) because solutions with positive deviation have weaker intermolecular forces, leading to a lower boiling point azeotrope.

Option A (If both assertion and reason are true and the reason is the correct explanation of the assertion) is correct because the definition of molality is accurately stated, and it directly explains the assertion.

Option A (Hydration energy > lattice energy) is correct because an exothermic dissolution process implies that the energy released during hydration is greater than the energy required to break the lattice.

Option B (2 M) is correct because the chloride ion concentration is twice the molarity of $CaCl_2$ due to each molecule dissociating into two chloride ions.

Option A ($4.6\;\mathrm{ }N$) is correct because Normality is calculated by multiplying Molarity by the basicity of the acid.

Option C (Associated) is correct because the depression in freezing point is inversely proportional to the van't Hoff factor, indicating association.

Option A (Two sucrose solution of same molality prepared in different solvent will have the same freezing point depression) is false because the freezing point depression depends on the cryoscopic constant ($k_f$) of the solvent, which varies for different solvents.

Option A (Victor Meyer’s method) is correct because it is used to determine the molecular weight of volatile solutes, not non-volatile solutes.

Answer 2 is correct because the equilibrium constant for the reverse reaction is the inverse of the square root of the original equilibrium constant.

Option B (Carbon disulphide-acetone) is correct because the intermolecular forces between CS2 and acetone are weaker than the forces within each pure liquid, leading to positive deviation.

Option D ($150 {~g}$) is correct because it is calculated using Raoult's law for vapor pressure lowering, considering the mole fraction of the solute.

Option A (Vapour pressure) is correct because vapor pressure itself is not a colligative property, but the *lowering* of vapor pressure is.

Option D (A supersaturated solution) is correct because a supersaturated solution is a metastable system that can easily precipitate upon disturbance.

Option A is correct because for an ideal solution, the volume change upon mixing is zero, which directly explains why the total volume is the sum of individual volumes.

Option D is correct because adding NaCl to water decreases vapor pressure, and the addition of a non-volatile solute also decreases vapor pressure, making both the assertion and the reason incorrect.