Question

To calculate the freezing point of an ideal dilute solution of a single, nondissociating solute of a solvent, the minimum information one must know is: a. the same quantities as in B, plus the freezing point of the pure solvent b. the molality (of the solute) and the freezing point depression constant of the solvent c. all of the quantities in C, plus the weight of the solvent d. all of the quantities in C, plus the molecular weight of the solute e. the molality (of the solute)

Answer 1

Answer:

the same quantities as in B, plus the freezing point of the pure solvent

Explanation:

Using the formula;

∆T = K· m. i

Where;

∆T = freezing point depression of the solution

K = freezing point depression constant

m = molality of the solution

i = vant Hoff factor

Since the solute is a single, non-dissociating solute, i=1

The equation reduces to;

∆T = K· m

So we must know the freezing point depression constant and the molality of the solution.

In addition; ∆T = freezing point of pure solvent- freezing point of solution

Hence, if we use the formula, ∆T = K· m to calculate ∆T, then we must also know the value of the freezing point of pure solvent in order to compute the freezing point of the solution.