If 2.500 g of copper (II) chloride was added to 150.0 mL of a 0.500 M copper (II) chloride solution, what is the concentration of the new solution

0.624 M

Explanation:

Step 1: Calculate the moles of copper (II) chloride in the initial solution

We had 150.0 mL of a 0.500 M copper (II) chloride solution. The moles of copper (II) chloride present were:

0.1500 L × 0.500 mol/L = 0.0750 mol

Step 2: Calculate the moles of copper (II) chloride added (2.500 g)

The molar mass of copper (II) chloride is 134.45 g/mol.

2.500 g × (1 mol/134.45 g) = 0.01859 mol

Step 3: Calculate the total number of moles of solute in the final solution

0.0750 mol + 0.01859 mol = 0.0936 mol

Step 4: Calculate the molarity of the final solution

M = 0.0936 mol / 0.1500 L = 0.624 M

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