A dilute ferrous sulphate solution was gradually added to the
beaker containing acidified permanganate solution. The light
purple colour of the solution fades and finally disappears.
Which of the following is the correct explanation for the
observation?
(a) KMnO4
is an oxidising agent, it oxidises FeSO4
(b) FeSO4
acts as an oxidising agent and oxidises KMnO4
(c) The colour disappears due to dilution; no reaction is involved
(d) KMnO4
is an unstable compound and decomposes in presence
of FeSO4
to a colourless compound.
Answers
Answered by
5
A) is correct
The pink colour is due to Mn2+(KMnO4-oxidising agent ) , as FeSO4 is added KMnO4 oxidises Fe2+ to Fe3+ and itself gets reduced to MnO2
SO42- remains unchanged as it is already in its highest state of oxidation and cannot undergo further oxidation
Redox reaction occurs
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The pink colour is due to Mn2+(KMnO4-oxidising agent ) , as FeSO4 is added KMnO4 oxidises Fe2+ to Fe3+ and itself gets reduced to MnO2
SO42- remains unchanged as it is already in its highest state of oxidation and cannot undergo further oxidation
Redox reaction occurs
(Mark as brainliest!!)
Answered by
2
Answer:
option a is correct hope it helps
Explanation:
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