I want to produce a solution, which contains $0.02~\mathrm{mol~L}^{-1}~\mathrm{Cu}^{2+}$ and $~0.2~\mathrm{mol~L}^{-1}~\mathrm{NH}_3$. The following substances are given:
- copper(II) sulfate pentahydrate
- $100~\mathrm{mL~H}_2\mathrm{O}$
- diluted ammonia solution with a concentration of $2~\mathrm{mol~L}^{-1}$.
I need to determine the required volume ($V$) of $\mathrm{NH}_3$ and the mass ($m$) of $\mathrm{CuSO}_4\cdot 5\mathrm{H}_2\mathrm{O}$.
I have no idea how to calculate $m$. However, to calculate $V$, I solved the following system of equations:
$\dfrac{2~\mathrm{mol}}{\mathrm{L}} = \dfrac{n}{V}$
$\dfrac{0.2~\mathrm{mol}}{\mathrm{L}} = \dfrac{n}{V+0.1~\mathrm{L}}$
Therefore, $V = 0.01111~\mathrm{L}$. Is this correct?
Is $m=555~\mathrm{mg}$ correct?