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I was following the guide “Stoichiometric Determination: Empirical Formula of Copper Chloride”. Under the Procedure section the following reaction is given:

Producing solid $\ce{Cu}$ from a $\ce{Cu(II)}$ solution by reaction with $\ce{Zn}$.

$$\ce{\underset{(blue)}{Cu_xCl_y(aq)} + Zn(s) ->\underset{colorless}{ZnCl2(aq)} + Cu(s)}$$

If the decanted solution is not colorless, how would it affect the procedure and what does that indicate?

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    $\begingroup$ If the decanted solution is not colorless (say light bluish), it means reaction is not completed and $\ce{Cu}$ ions are still in the solution. So, your calculations would be off, because it is depend on the weight of $\ce{Cu}$ metal you isolated. $\endgroup$ – Mathew Mahindaratne Jul 11 at 22:03

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