Each copper(II) sulfate unit is associated with five water
Chapter 8, Problem 32QP(choose chapter or problem)
When copper(II) sulfate pentahydrate \(\left(\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}\right)\) is heated in air above \(100^{\circ} \mathrm{C}\), it loses the water molecules and its blue color:
\(\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{CuSO}_4+5 \mathrm{H}_2 \mathrm{O}\)
If \(9.60 \mathrm{~g}\) of \(\mathrm{CuSO}_4\) are left after heating \(15.01 \mathrm{~g}\) of the blue compound, calculate the number of moles of \(\mathrm{H}_2 \mathrm{O}\) originally present in the compound.
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