What is the concentration in molarity of a 1.32 L solution that contains 22.5 g of dissolved copper (II) chloride?

Question

If anyone could help it would be nice :). So, I understand to get the concentration in molarity you would need to make 22.5 grams of copper II chloride over the 1.32 solution, multiplying that by 1 mol copper II chloride over the molar mass (134.45), however this didn't give me the right answer. So would you need to add on the density of copper II chloride, with the given numbers available to find, 17.05 or use the density, 3.39 found on google, since density isn't clearly stated in the problem?

Answer 1

You shouldn't need to use density at all given the information provided in the problem. Not sure exactly what your math looked like to get an incorrect answer, but here is the simple way to solve this problem.

Molarity = moles of solute per liter of solution.

Liters of solution = 1.32 L (given in the problem)

Moles of copper(II) chloride = 22.5 g x 1 mol / 134.45 g = 0.1673 moles

Molarity of CuCl₂ = 0.1673 moles / 1.32 L = 0.127 M (3 sig.figs.)