So I'm facing a small chemistry problem that I can't find a way to solve. I'm not looking for answers, I'm just looking for how can I approach this problem.
The problem is as follows :
We put 5 g of non-pure zinc (with some impurities) into a 200 ml solution containing hydronium ions. At the end, we get some gases and we are left with 0.05 mol of hydronium ions in the solution.
Find the pure mass of zinc in that non-pure 5 g of zinc.
I really don't have any idea how to approach this problem. I have written and balanced the chemical equation:
$$\ce{Zn + 2H^+ = Zn^{2+} + H2}$$
I've arrived at the above equation from redox half-reactions. From here I don't know where to go.
Generally I would use the degree of purity formula:
$$P = \frac{C\cdot M}{10\cdot d}$$
where $P$ is degree of purity, $C$ is concentration, $M$ is the molar mass, and $d$ is the density, but this one is used for gases and liquids only. Besides, we've never studied how to compute the density of a metal.