Question

The freezing point of a solution containing 0.4 g acetic acid in 40 g of benzene

Answer 1

The freezing point of solution is 4.64°C

Explanation:

Depression in freezing point is defined as the difference in the freezing point of water and freezing point of solution.

$\Delta T_f=\text{Freezing point of benzene}-\text{Freezing point of solution}$

To calculate the depression in freezing point, we use the equation:

$\Delta T_f=iK_fm$

Or,

$\text{Freezing point of benzene}-\text{Freezing point of solution}=iK_f\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}$

where,

Freezing point of benzene = 5.5°C

$m_{solute}$ = Given mass of solute (acetic acid) = 0.4 g

$M_{solute}$ = Molar mass of solute (acetic acid) = 60 g/mol

$W_{solvent}$ = Mass of solvent (benzene) = 40 g

$K_f$ = molal freezing point depression constant = 5.12°C/m

i = 1 (non-electrolytes)

Putting values in above equation:

$5.5-\text{Freezing point of solution}=1\times 5.15\times \frac{0.4\times 1000}{60\times 40}\\\\\text{Freezing point of solution}=4.64^oC$

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