Chemistry

Redox Reactions

Redox reactions as the basis for titration

{MnO}_{4}{ }^{-}ions are reduced in acidic condition to {Mn}^{

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Solving time: 4 mins

$MnO_{4}^{-}$ ions are reduced in acidic condition to $Mn^{2 +}$ ions whereas they are reduced in neutral condition to $MnO_{2}$ . The oxidation of $25 ml$ of a solution $X$ containing $Fe^{2 +}$ ions required in acidic condition $20 ml$ of a solution $Y$ containing $MnO_{4}^{-}$ ions. What volume (in mL) of solution $Y$ would be required to oxidise $25 ml$ of solution $X$ containing $Fe^{2 +}$ ions in neutral condition? (Report answer upto one decimal place)

Name: Video answer for MnO4−ions are reduced in acidic condition to Mn2+ ions whereas they are reduced in neutral condition to MnO2. The oxidation of 25ml of a solution X containing Fe2+ ions required in acidic condition 20ml of a solution Y containing MnO4−ions. What volume (in mL) of solution Y would be required to oxidise 25ml of solution X containing Fe2+ ions in neutral condition? (Report answer upto one decimal place)
Uploaded: 2022-08-22T10:50:51.000Z
Duration: 6 min

Views: 5,770 students

Updated on: Aug 22, 2022

Text solutionVerified

In acidic medium,

M n + 7 O_{4}^{-} \to M n^{+ 2}

Change in oxidation number = 5

N_{1} V_{1} \equiv N_{2} V_{2}

Fe^{2 +} MnO_{4}^{-}

N \times 25 \equiv 5 M \times 20

25 N \equiv 100 M (i)

In neutral medium,

M n + 7 O_{4}^{-} \to M n + 4 O_{2}

Change in oxidation number =3

N_{1} V_{1} Fe^{2 +} 25 \times N 25 N \equiv N_{2} V_{2} MnO_{4}^{-} \equiv 3 M \times V \equiv 3 M V (ii)

(For

MnO_{4}^{-}, N = 3 M

in neutral medium)
Equating

(i)

and

(ii)

100 M = 3 M \times V

V = \frac{100}{3} = 33.3 mL

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Amelia Discussed

MnO_{4}^{-}

ions are reduced in acidic condition to

Mn^{2 +}

ions whereas they are reduced in neutral condition to

MnO_{2}

. The oxidation of

25 ml

of a solution

X

containing

Fe^{2 +}

ions required in acidic condition

20 ml

of a solution

Y

containing

MnO_{4}^{-}

ions. What volume (in mL) of solution

Y

would be required to oxidise

25 ml

of solution

X

containing

Fe^{2 +}

ions in neutral condition? (Report answer upto one decimal place)

12 mins ago

Discuss this question LIVE

12 mins ago

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Question Text	$MnO_{4}^{-}$ ions are reduced in acidic condition to $Mn^{2 +}$ ions whereas they are reduced in neutral condition to $MnO_{2}$ . The oxidation of $25 ml$ of a solution $X$ containing $Fe^{2 +}$ ions required in acidic condition $20 ml$ of a solution $Y$ containing $MnO_{4}^{-}$ ions. What volume (in mL) of solution $Y$ would be required to oxidise $25 ml$ of solution $X$ containing $Fe^{2 +}$ ions in neutral condition? (Report answer upto one decimal place)
Updated On	Aug 22, 2022
Topic	Redox Reactions
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 1
Upvotes	135
Avg. Video Duration	6 min

Text solutionVerified

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