We’re being asked to calculate the freezing temperature of a solution of 115.0 g of sucrose, C_{12}H_{22}O_{11}, in 350.0 g of water. When calculating the freezing point of a solution, we’re going to use the equation for Freezing Point Depression.

$\overline{){\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{=}}{\mathbf{i}}{\mathbf{\xb7}}{{\mathbf{K}}}_{{\mathbf{f}}}{\mathbf{\xb7}}{\mathbf{m}}}$

∆T_{f} = change in freezing point = T_{f pure solvent} –T_{f solution}

K_{f} = freezing point depression constant

i = van' t Hoff factor of the solute = no. of ions

m = molality

We're going to calculate the freezing point of the solution using the following steps:

**Step 1:** Calculate the moles of solute.**Step 2:** Calculate the molality of the solution.**Step 3:** Calculate the change in temperature (ΔT_{f}).**Step 4:** Calculate the freezing point of the solution.

**Step 1:** Calculate the moles of solute (sucrose).

What is the freezing temperature of a solution of 115.0 g of sucrose, C _{12}H_{22}O_{11}, in 350.0 g of water, which freezes at 0.0 °C when pure?

(a) Outline the steps necessary to answer the question.

(b) Answer the question.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.