# Problem: A solution is prepared by dissolving 456 g of sucrose (C12H22O11, molar mass 342 g/mol) in 764 g of water (18.02 g/mol; density 1.00 g/mL) calculate:d) How many grams of Ca 3 (PO4)2 must be added to 764g of water to have the same effect?

###### FREE Expert Solution

We’re being asked to calculate the mass of Ca3(PO4)needed to achieve the freezing point of the solution as the one given with sucrose.

Recall that the freezing point of a solution is lower than that of the pure solvent and the change in freezing point (ΔT­f) is given by:

The change in freezing point is also related to the molality of the solution:

$\overline{){{\mathbf{\Delta T}}}_{{\mathbf{f}}}{\mathbf{=}}{{\mathbf{imK}}}_{{\mathbf{f}}}}$

where:

i = van’t Hoff factor

m = molality of the solution (in m or mol/kg)

Kf = freezing point depression constant (in ˚C/m) of the solvent

We go through the following steps to solve the problem:

Step 1. Calculate the molality of the solution

Step 2. Calculate the moles of the solute

Step 3. Calculate the mass of the solute

80% (49 ratings)
###### Problem Details

A solution is prepared by dissolving 456 g of sucrose (C12H22O11, molar mass 342 g/mol) in 764 g of water (18.02 g/mol; density 1.00 g/mL) calculate:

d) How many grams of Ca (PO4)must be added to 764g of water to have the same effect?

Frequently Asked Questions

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 The Colligative Properties concept. You can view video lessons to learn The Colligative Properties. Or if you need more The Colligative Properties practice, you can also practice The Colligative Properties practice problems.