In going from the top to the bottom of the activity series below, the ease of oxidation of the metal __________, which means that __________

\begin{array}{l}\text { An Activity Series for Metals in Aqueous Solution }\\\begin{array} { | l l | } \hline \text { Metal } & \text { Oxidation Reaction } \\\hline \text { Lithium } & \mathrm { Li } ( s ) \rightarrow \mathrm { Li } ^ { + } ( a q ) + \mathrm { e } ^ { - } \\\hline \text { Potassium } & \mathrm { K } ( s ) \rightarrow \mathrm { K } ^ { + } ( a q ) + \mathrm { e } ^ { - } \\\hline \text { Barium } & \mathrm { Baa } ( s ) \rightarrow \mathrm { Ba } ^ { 2 + } ( a q ) + 2 \mathrm { e } ^ { - } \\\hline \text { Calcium } & \mathrm { Ca } ( i ) \rightarrow \mathrm { Ca } ^ { 2 + } ( a q ) + 2 \mathrm { e } ^ { - } \\\hline \text { Sodium } & \mathrm { Na } ( s ) \rightarrow \mathrm { Na } ^ { + } ( a q ) + \mathrm { e } ^ { - } \\\hline \text { Magnesium } & \mathrm { Mg } ( s ) \rightarrow \mathrm { Mg } ^ { 2 + } ( a q ) + 2 \mathrm { e } ^ { - } \\\hline \text { Aluminum } & \mathrm { Al } ( s ) \rightarrow \mathrm { Al } ^ { 3 + } ( a g ) + 3 \mathrm { e } ^ { - } \\\hline \text { Manganese } & \mathrm { Mn } ( s ) \rightarrow \mathrm { Mn } ^ { 2 + } ( a q ) + 2 \mathrm { e } ^ { - } \\\hline \text { Zinc } & \mathrm { Zn } ( s ) \rightarrow \mathrm { Zn } ^ { 2 + } ( a q ) + 2 \mathrm { e } ^ { - } \\\hline \text { Chromium } & \mathrm { Cr } ( g ) \rightarrow \mathrm { Cr } ^ { 3 + } ( a q ) + 3 \mathrm { e } ^ { - } \\\hline\end{array}\end{array}

A) increases, magnesium can reduce zinc ions.
B) increases, magnesium ions can oxidize zinc.
C) decreases, zinc can reduce magnesium ions.
D) increases. zinc ions can oxidize magnesium.
E) decreases, magnesium can reduce zinc ions.

Determine the Molar Concentration of an Aqueous Solution of Lead(II)

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