# A). To what volume should you dilute 121 mL of an 8.00 M CuCl2 solution so that 52.0 mL of the...

## Question:

A). To what volume should you dilute 121 mL of an 8.00 M CuCl2 solution so that 52.0 mL of the diluted solution contains 4.44 g CuCl2?

B). Silver nitrate solutions are often used to plate silver onto other metals. What is the maximum amount of silver (in grams) that can be plated out of 5.1 L of an AgNO3 solution containing 3.4 % Ag by mass? Assume that the density of the solution is 1.01 g/mL. Express your answer using two significant figures. C). An aqueous solution containing 35.6 g of an unknown molecular (non-electrolyte) compound in 149.9 g of water was found to have a freezing point of -1.3 C.

Calculate the molar mass of the unknown compound.

Express your answer using two significant figures.

## Freezing Point Depression:

When a solute is dissolved in a solvent, the vapor pressure of the solvent decreases. As a result, its freezing point also decreases. The lowering of the freezing point of the solution is directly proportional to the molality of the solution. This is expressed in the formula below:

{eq}\Delta T_f=-mK_f {/eq}

where {eq}\Delta T_f {/eq} is the change in the freezing point of the solvent, {eq}m {/eq} is the molality of the solution and {eq}K_f {/eq} is the molal freezing point depression constant of the solvent.

## Answer and Explanation: 1

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A). The concentration of CuCl{eq}_2 {/eq} when 52.0 mL solution contains 4.44 g CuCl{eq}_2 {/eq} is:

{eq}\rm \dfrac{4.44 \:g \:CuCl_2}{52.0...

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Chapter 8 / Lesson 6Colligative properties are important to determine molar mass as related to vapor pressure, boiling point, freezing point, and osmotic pressure. Examine freezing point depression to understand the process for finding molar mass.