Question #117672
Consider the following reaction: Cr2O72– + 6Br– + 14 H+ à 2 Cr3+ + 3Br2 + 7H2O
In a redox titration, 14.62 mL of 0.175 M Cr2O72– was needed to completely react with a 25.00 mL sample of Br–. Calculate the [Br–] in the original solution.
1
Expert's answer
2020-05-24T03:10:34-0400

In the reaction

Cr2O72– + 6Br + 14 H+ \rightarrow 2 Cr3+ + 3Br2 + 7H2O,

1 ion of Cr2O72– reacts with 6 ions of Br-, therefore their number of the moles relate as:

n(Cr2O72)=n(Br)6n(Cr_2O_7^{2–}) = \frac{n(Br^-)}{6} .

The number of the moles of the bichromate anion is:

n(Cr2O72)=cV=14.621030.175=2.559103n(Cr_2O_7^{2–}) = cV = 14.62·10^{-3}·0.175 = 2.559·10^{-3} mol.

The number of the moles in 25.000 mL sample of Br- is:

n(Br)=62.559103=0.0154n(Br^-) = 6·2.559·10^{-3} = 0.0154 mol.

Finally, the concentration of Br- in the original solution is the ratio of the number of the moles of Br- that react in titration to the volume of the sample:

c(Br)=nV=0.015425103=0.614c(Br^-) = \frac{n}{V} = \frac{0.0154}{25·10^{-3}} = 0.614 M.

Answer: the Br- concentration in the original solution is 0.614 M.


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