AP Chemistry
1.3 Elemental Composition of Pure Substances
A student performs a laboratory experiment to determine the value of \(x\) in the formula of hydrated copper(II) sulfate, \(\text{CuSO}_4 \cdot x\text{H}_2\text{O}\). A sample of the hydrate is placed in an open crucible and heated strongly to drive off all the water of hydration according to the following equation:
\[ \text{CuSO}_4 \cdot x\text{H}_2\text{O}(s) \rightarrow \text{CuSO}_4(s) + x\,\text{H}_2\text{O}(g) \]
During heating, some of the solid splatters out of the crucible and is lost. If the student does not notice this loss and uses the final mass of the crucible and residue to calculate \(x\), how will the calculated value of \(x\) compare to the actual value, and why?
\[ \text{CuSO}_4 \cdot x\text{H}_2\text{O}(s) \rightarrow \text{CuSO}_4(s) + x\,\text{H}_2\text{O}(g) \]
During heating, some of the solid splatters out of the crucible and is lost. If the student does not notice this loss and uses the final mass of the crucible and residue to calculate \(x\), how will the calculated value of \(x\) compare to the actual value, and why?
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