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in a virtual lab: redox of Mn
0.01 M KMnO4 is added to 3 different solutions:
1) acidified solution: H2SO3 + NaHSO3 + KMnO4 = ?
2) control solution: NaHSO3 + KMnO4 = ?
3) basified solution: NaOH + NaHSO3 + KMnO4 = ?
I need help figuring out what the products of these 3 reactions will be...
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The oxidation state of manganese in potassium permanganate is +7, which is reduced by `NaHSO_3` to different degrees to form various oxidation states, and corresponding colour changes are observed.
In neutral solution (control), orange colour is observed due to the formation of `MnO_2` .
In the basified solution, green colour due to `Mn^(+7)` is observed.
In the acidic solution, a faint pink colur is obtainable due to the formation of `Mn^(2+)` ions.
The balanced chemical reactions are as follows:
`3NaHSO_3 + 2KMnO_4 +NaOH rarr K_2SO_4 + 2Na_2SO_4 + 2MnO_2(s) + 2H_2O`
`NaHSO_3 + 3 NaOH + 2 KMnO_4 rarr Na_2SO-4 + Na_2MnO_4 + K_2MnO_4 + 2H_2O`
`4NaHSO_3 + H_2SO_3 + 2KMnO_4 rarr K_2SO_4 + 2Na_2SO_4 + 2MnSO_4 +3H_2O`
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