Suppose 40.8g of copper(II) acetate is dissolved in 200.mL of a 0.70 M aqueous solution of sodium chromate. Calculate the final molarity of copper(II) cation in the solution. You can assume the volume of the solution doesn't change when the copper(II) acetate is dissolved in it.
Be sure your answer has the correct number of significant digits.

0.42 M

Explanation:

The reaction that takes place is:

First we calculate the moles of Na₂CrO₄, using the given volume and concentration:

(200 mL = 0.200L)

Now we calculate the moles of Cu(CH₃COO)₂, using its molar mass:

Because the molar ratio of Cu(CH₃COO)₂ and Na₂CrO₄ is 1:1, we can directly substract the reacting moles of Na₂CrO₄ from the added moles of Cu(CH₃COO)₂:

Finally we calculate the resulting molarity of Cu⁺², from the excess cations remaining:

c. is the answer

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