Why is the oxidation of $M n^{2 +}$ $Mn^(2+)$ in ACIDIC media represented differently to the oxidation of $M n^{2 +}$ $Mn^(2+)$ in an ALKALINE medium? What do we mean by $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ ?

Question

Why is the oxidation of $M n^{2 +}$ $Mn^(2+)$ in ACIDIC media represented differently to the oxidation of $M n^{2 +}$ $Mn^(2+)$ in an ALKALINE medium? What do we mean by $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ ?

1 Answer

Impact of this question

2198 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-03-24T08:47:27

Because chemistry follows experiment...........

Explanation:

$H^{+}$ $H^+$ is very much a conceptual particle. When we write $H^{+}$ $H^+$ in a reaction we mean the hydronium ion, $H_{3} O^{+}$ $H_3O^+$ , which AGAIN is a conceptual species. The actual species is (probably) a cluster of 3-4 water molecules, with an extra proton to give $H_{7} O_{3}^{+}$ $H_7O_3^+$ , or $H_{9} O_{4}^{+}$ $H_9O_4^+$ . The clusters exchange the proton between themselves. We write $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ for convenience.

When we write a redox equation, of course we balance mass and charge, and the use of $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ is a means to this end. It happens that in ACIDIC medium, $M n^{2 +}$ $Mn^(2+)$ , may be oxidized to $M n O_{4}^{-}$ $MnO_4^(-)$ :

$M n^{2 +} + 4 H_{2} O \to M n O_{4}^{-} + 8 H^{+} + 5 e^{-}$ $Mn^(2+) +4H_2O rarr MnO_4^(-) + 8H^(+) + 5e^-$

In alkaline media, $M n^{2 +}$ $Mn^(2+)$ may be oxidized to $manganate ion$ $"manganate ion"$ , $M n O_{4}^{2 -}$ $MnO_4^(2-)$ , which is $M n (V I +)$ $Mn(VI+)$ :

$M n^{2 +} + 8 H O^{-} \to M n O_{4}^{2 -} + 4 H_{2} O + 4 e^{-}$ $Mn^(2+) +8HO^(-) rarr MnO_4^(2-) + 4H_2O + 4e^-$

$Manganates$ $"Manganates"$ give green salts.

Mass and charge are balanced (I think) as required. Note that this representation follows the actual experiment, not vice versa.

If there is a further issue or query, fire away.

Science

Math

Humanities

... and beyond

Why is the oxidation of $M n^{2 +}$ $Mn^(2+)$ in ACIDIC media represented differently to the oxidation of $M n^{2 +}$ $Mn^(2+)$ in an ALKALINE medium? What do we mean by $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ ?

1 Answer

Explanation:

Related questions

Impact of this question

Science

Math

Humanities

... and beyond

Why is the oxidation of Mn2+Mn^(2+) in ACIDIC media represented differently to the oxidation of Mn2+Mn^(2+) in an ALKALINE medium? What do we mean by H+H^+ or H3O+H_3O^+?

1 Answer

Explanation:

Related questions

Impact of this question

Why is the oxidation of $M n^{2 +}$ $Mn^(2+)$ in ACIDIC media represented differently to the oxidation of $M n^{2 +}$ $Mn^(2+)$ in an ALKALINE medium? What do we mean by $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ ?