# Problem: What is the freezing temperature of a solution of 115.0 g of sucrose, C 12H22O11, 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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###### FREE Expert Solution

We’re being asked to calculate the freezing temperature of a solution of 115.0 g of sucrose, C12H22O11, 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.

$\overline{){\mathbf{∆}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{=}}{\mathbf{i}}{\mathbf{·}}{{\mathbf{K}}}_{{\mathbf{f}}}{\mathbf{·}}{\mathbf{m}}}$

∆Tf = change in freezing point = Tf pure solvent –Tf solution
Kf = 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 (ΔTf).
Step 4: Calculate the freezing point of the solution.

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

96% (209 ratings) ###### Problem Details

What is the freezing temperature of a solution of 115.0 g of sucrose, C 12H22O11, 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.