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A student determines the copper(II) content of a solution by first precipitating it as copper(II) hydroxide, and then decomposing the hydroxide to copper(II) oxide by heating. How many grams of copper(II) oxide should the student obtain if his solution contains 40.0 mL of 0.462 M copper(II) nitrate?

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Answer:

1.44g of CuO

Explanation:

First we put down the balanced chemical reaction equations involved. Then we obtain the amount of Cu2+ present in the Cu(NO3) from the information provided. This same amount of Cu2+ is present in Cu(OH)2 which decomposes to give copper II oxide. From the balanced reaction equation, we obtain the mass of CuO obtained from this amount of Cu2+ as shown in the image attached.

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