An experiment was performed to investigate the reaction between $\mathrm{Ln}$ metal and $\mathrm{Ni}^{2+}(a q)$ at different concentrations. Because the $\mathrm{Ni}^{2+}(a q)$ ion is green, the extent of the reaction was determined using spectrophotometric analysis. Four $20.0 \mathrm{~mL}$ standard solutions of $\mathrm{Ni}^{2+}(a q)$ were prepared by dissolving $\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}$ (molar mass $240 \mathrm{~g} / \mathrm{mol}$ ) in water. The absorbance of each solution was measured; the results are shown both in the table below and in the following plot of the absorbance data.
\begin{tabular}{|c|c|c|}
\hline Solution & {$\left[\mathrm{Ni}^{2+} ight]$} & Absorbance \
\hline 1 & 0.020 & 0.12 \
\hline 2 & 0.040 & 0.25 \
\hline 3 & 0.060 & 0.39 \
\hline 4 & 0.080 & 0.51 \
\hline
\end{tabular}
15. Which species is being oxidized in the reaction between $\mathrm{Zn}$ metal and $\mathrm{NiCl}_{2}(a q)$ ?
(A) $\mathrm{Zn}$
(B) $\mathrm{Zn}^{2+}$
(C) $\mathrm{Ni}$
(D) $\mathrm{Ni}^{2+}$
Page

Question

An experiment was performed to investigate the reaction between $\mathrm{Ln}$ metal and $\mathrm{Ni}^{2+}(a q)$ at different concentrations. Because the $\mathrm{Ni}^{2+}(a q)$ ion is green, the extent of the reaction was determined using spectrophotometric analysis. Four $20.0 \mathrm{~mL}$ standard solutions of $\mathrm{Ni}^{2+}(a q)$ were prepared by dissolving $\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}$ (molar mass $240 \mathrm{~g} / \mathrm{mol}$ ) in water. The absorbance of each solution was measured; the results are shown both in the table below and in the following plot of the absorbance data.
\begin{tabular}{|c|c|c|}
\hline Solution & {$\left[\mathrm{Ni}^{2+}ight]$} & Absorbance \
\hline 1 & 0.020 & 0.12 \
\hline 2 & 0.040 & 0.25 \
\hline 3 & 0.060 & 0.39 \
\hline 4 & 0.080 & 0.51 \
\hline
\end{tabular}
15. Which species is being oxidized in the reaction between $\mathrm{Zn}$ metal and $\mathrm{NiCl}_{2}(a q)$ ?
(A) $\mathrm{Zn}$
(B) $\mathrm{Zn}^{2+}$
(C) $\mathrm{Ni}$
(D) $\mathrm{Ni}^{2+}$
Page

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Identify the species involved in oxidation and reduction**: In a redox reaction, the species that gets oxidized loses electrons, while the species that gets reduced gains electrons. ‖ ‖ 2 ⋮ **Analyze the possible reactions**: $\mathrm{Zn}$ can be oxidized to $\mathrm{Zn}^{2+}$ by losing two electrons ($\mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2e^{-}$). $\mathrm{Ni}^{2+}$ can be reduced to $\mathrm{Ni}$ by gaining two electrons ($\mathrm{Ni}^{2+} + 2e^{-} \rightarrow \mathrm{Ni}$). ‖ ‖ 3 ⋮ **Determine the species being oxidized**: Since $\mathrm{Zn}$ metal can lose electrons to form $\mathrm{Zn}^{2+}$, it is the species that is being oxidized in the reaction with $\mathrm{NiCl}_{2}(aq)$. ‖ ∻Answer∻ ⚹ (A) $\mathrm{Zn}$ ⚹ ∻Key Concept∻ ⚹ Oxidation in a redox reaction ⚹ ∻Explanation∻ ⚹ In the reaction between $\mathrm{Zn}$ metal and $\mathrm{NiCl}_{2}(aq)$, $\mathrm{Zn}$ is oxidized to $\mathrm{Zn}^{2+}$ as it loses electrons. ⚹◊What is the redox reaction taking place between $Zn$ metal and $NiCl_2(aq)$?⍭ Generate me a similar question◊

Sia