# 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.

## 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.