9.) Calculate the normality of $\mathrm{Cu}^{2+}$ in a solution that is made by dissolving $8.77 \mathrm{~g}$ of $\mathrm{Au}\left(\mathrm{NO}_{3}\right)_{3}$ in enough water to make $175 \mathrm{~mL}$ of solution after excess copper metal is added to the solution. The relevant reaction is
$$
3 \mathrm{Cu}(s)+2 \mathrm{Au}^{3+}(a q) \rightarrow 2 \mathrm{Au}(s)+3 \mathrm{Cu}^{2+}(a q)
$$

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Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Calculate moles of Au(NO3)3**: First, we need to calculate the moles of $\mathrm{Au(NO_3)_3}$ using its molar mass. The molar mass of $\mathrm{Au(NO_3)_3}$ is $197.0 + 3 \times (14.0 + 3 \times 16.0)$ g/mol. ‖ ‖ 2 ⋮ **Moles of Au(NO3)3**: Using the mass of $\mathrm{Au(NO_3)_3}$ given, $8.77 \text{ g}$, we find the moles by dividing by the molar mass. ‖ ‖ 3 ⋮ **Stoichiometry of reaction**: According to the balanced chemical equation $3\mathrm{Cu(s)} + 2\mathrm{Au^{3+}(aq)} \rightarrow 2\mathrm{Au(s)} + 3\mathrm{Cu^{2+}(aq)}$, 2 moles of $\mathrm{Au^{3+}}$ produce 3 moles of $\mathrm{Cu^{2+}}$. ‖ ‖ 4 ⋮ **Calculate moles of Cu2+**: Using the stoichiometry from the balanced equation, calculate the moles of $\mathrm{Cu^{2+}}$ produced from the moles of $\mathrm{Au(NO_3)_3}$ dissolved. ‖ ‖ 5 ⋮ **Calculate normality**: Normality ($N$) is defined as the equivalent of solute per liter of solution. Since each mole of $\mathrm{Cu^{2+}}$ provides 2 equivalents (due to its +2 charge), we multiply the moles of $\mathrm{Cu^{2+}}$ by 2 to get the equivalents. Then, we divide by the volume of the solution in liters to find the normality. ‖ ∻Answer∻ ⚹ [Insert final answer here] ⚹ ∻Key Concept∻ ⚹ Normality is a measure of concentration that is equivalent to the molarity multiplied by the number of equivalents per mole of solute. In the case of $\mathrm{Cu^{2+}}$, each mole has 2 equivalents. ⚹ ∻Explanation∻ ⚹ To find the normality of $\mathrm{Cu^{2+}}$ in the solution, we calculate the moles of $\mathrm{Au(NO_3)_3}$, use the stoichiometry of the reaction to find the moles of $\mathrm{Cu^{2+}}$ produced, and then calculate the equivalents of $\mathrm{Cu^{2+}}$ in the final solution volume. ⚹◊What is the normality of Cu2+ in the solution after excess copper metal is added?⍭ Generate me a similar question◊

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