A solution containing 2-7 - 10-3 mol of A2- ions required 1-6 - 10-3 mole of MnO4- for the oxidation of A2- to AO3- the medium used is-

The correct option is B Acidic 2KMnO_4 #8203;+3H_2 #8203;SO_4 #8203;→ K_2 #8203;SO_4 #8203;+2MnSO_4 #8203;+3H_2 #8203;O+5[O] Hence the medium ...

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Byju's Answer

Standard XII

Chemistry

Hydrochloric Acid

A solution co...

Question

A solution containing $2.7 \times 10^{- 3}$ mol of $A^{2 +}$ ions required $1.6 \times 10^{- 3}$ mole of $M n O_{4}^{-}$ for the oxidation of $A^{2 +}$ to $A O_{3}^{-}$ the medium used is:

Neutral

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Acidic

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Strong basic

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None of these

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Solution

The correct option is B Acidic
$2 K M n O_{4} + 3 H_{2} S O_{4} \to K_{2} S O_{4} + 2 M n S O_{4} + 3 H_{2} O + 5 [O]$
Hence the medium used is acidic.
Option B is correct

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Similar questions

2.68 \times 10^{- 3} m o l

of a solution containing an ion

A^{n +}

required

1.6 \times 10^{- 3}

mol of

{M n O_{4}}^{- 1}

for oxidation of

A^{n +}

{A O_{3}}^{- 1}

ion in acid medium. What is the value of

n

Q. A solution containing

2.68 \times 10^{- 3} mol

A^{n +}

ions requires

1.61 \times 10^{- 3} mol

M n O_{4}^{-}

for the complete oxidation of

A^{n +}

A O_{3}^{-}

in acidic medium. What is the value of

n

2.68 \times 10^{- 3}

moles of a solution containing an ion

A^{n +}

require

1.61 \times 10^{- 3}

moles

M n O_{4}^{-}

for the oxidation of

A^{n +}

A O_{3}^{-}

in acid medium. What is the value of n?

2.68 \times 10^{- 3}

moles of a solution containing an ion

A^{n +}

require

1.61 \times 10^{- 3}

moles of

M n O_{4}^{-}

for the oxidation of

A^{n +}

A O_{3}^{-}

in acidic medium. What is the value of

n

Q. A solution containing

2.68 \times 10^{- 3} m o l

A^{n +}

ions requires

1.608 \times 10^{- 3} m o l

M n O_{4}^{-}

for the complete oxidation of

A^{n +}

A O_{3}^{-}

in acidic medium. What is the value of

n

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A solution containing 2.7×10−3 mol of A2+ ions required 1.6×10−3 mole of MnO−4 for the oxidation of A2+ to AO−3 the medium used is:

The correct option is B Acidic2KMnO4+3H2SO4→K2SO4+2MnSO4+3H2O+5[O]Hence the medium used is acidic. Option B is correct

A solution containing $2.7 \times 10^{- 3}$ mol of $A^{2 +}$ ions required $1.6 \times 10^{- 3}$ mole of $M n O_{4}^{-}$ for the oxidation of $A^{2 +}$ to $A O_{3}^{-}$ the medium used is:

The correct option is B Acidic
$2 K M n O_{4} + 3 H_{2} S O_{4} \to K_{2} S O_{4} + 2 M n S O_{4} + 3 H_{2} O + 5 [O]$
Hence the medium used is acidic.
Option B is correct