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Solved: Iron(II) can be oxidized by an acidic K2Cr2O7

Chapter 4, Problem 95P

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QUESTION:

Iron(II) can be oxidized by an acidic \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) solution according to the net ionic equation:

\(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+6 \mathrm{Fe}^{2+}+14 \mathrm{H}^{+} \stackrel{\longrightarrow}{2 \mathrm{Cr}^{3+}}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}\)

If it takes \(26.0 \mathrm{~mL}\) of \(0.0250 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to titrate \(25.0 \mathrm{~mL}\) of a solution containing \(\mathrm{Fe}^{2+}\), what is the molar concentration of \(\mathrm{Fe}^{2+}\)?

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QUESTION:

Iron(II) can be oxidized by an acidic \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) solution according to the net ionic equation:

\(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+6 \mathrm{Fe}^{2+}+14 \mathrm{H}^{+} \stackrel{\longrightarrow}{2 \mathrm{Cr}^{3+}}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}\)

If it takes \(26.0 \mathrm{~mL}\) of \(0.0250 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to titrate \(25.0 \mathrm{~mL}\) of a solution containing \(\mathrm{Fe}^{2+}\), what is the molar concentration of \(\mathrm{Fe}^{2+}\)?

ANSWER:

Step 1 of 3

The goal of the problem is to find the molar concentration of \(\mathrm{Fe}^{2+}\).

Given:

Volume of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}=26.0 \mathrm{~mL}\)

Molarity of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}=0.0250 \mathrm{M}\).

Given equation:

\(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+6 \mathrm{Fe}^{2+}+14 \mathrm{H}^{+} \rightarrow 2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}\)

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