Question #ddcdf
1 Answer
Here's what I got.
Explanation:
For starters, ignore the hydroxide anions present on the reactants' side, they will come into play later.
The half-reaction given to you describes the oxidation of chromium from an oxidation state of
#stackrel(color(blue)(+3))("Cr")("OH")_ 3 -> stackrel(color(blue)(+6))("Cr")"O"_4^(2-) + 3"e"^(-)#
Here one atom of chromium loses
Now, balance the oxygen atoms by adding water,
#"H"_ 2"O" + stackrel(color(blue)(+3))("Cr")("OH")_ 3 -> stackrel(color(blue)(+6))("Cr")"O"_4^(2-) + 3"e"^(-)#
Now focus on the hydrogen atoms. You have a total of
#"H"_ 2"O" + stackrel(color(blue)(+3))("Cr")("OH")_ 3 -> stackrel(color(blue)(+6))("Cr")"O"_4^(2-) + 3"e"^(-) + 5"H"^(+)#
Because you're in basic medium, the protons will be neutralized by hydroxide anions,
To keep the equation balanced, add
#5"OH"^(-) + "H"_ 2"O" + stackrel(color(blue)(+3))("Cr")("OH")_ 3 -> stackrel(color(blue)(+6))("Cr")"O"_4^(2-) + 3"e"^(-) + overbrace( 5"H"^(+) + 5"OH"^(-))^(color(darkgreen)(=5"H"_2"O"))#
The
#5"OH"^(-) + color(red)(cancel(color(black)("H"_ 2"O"))) + stackrel(color(blue)(+3))("Cr")("OH")_ 3 -> stackrel(color(blue)(+6))("Cr")"O"_4^(2-) + 3"e"^(-) + color(red)(cancel(color(black)(5)))^4"H"_2"O"#
Therefore, the balanced half-reaction will look like this
#color(green)(bar(ul(|color(white)(a/a)color(black)(5"OH"^(-) + "Cr"("OH")_ 3 -> "CrO"_ 4^(2-) + 4"H"_ 2"O" + 3"e"^(-))color(white)(a/a)|)))#