# 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.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Freezing Point Depression concept. If you need more Freezing Point Depression practice, you can also practice Freezing Point Depression practice problems.

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Based on our data, we think this problem is relevant for Professor Davis' class at UCF.

What textbook is this problem found in?

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.