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0.01 \; \mathrm{M}\; \mathrm{KMnO}_{4} solution was added to 20.0 \mathrm{~mL} \text { of } 0.05 \mathrm{M} \; \mathrm{Mohr} ' \mathrm{~s} salt solution through a burette. The initial reading of 50 mL burette is zero. The volume of \mathrm{KMnO}_{4} solution left in the burette after the end point is ________mL. (nearest integer)

Option: 1

30


Option: 2

-


Option: 3

-


Option: 4

-


Answers (1)

best_answer

The formula for Mohr's Salt is \mathrm{\left( NH _{4}\right)_{2}SO_4\cdot Fe \left( SO _{4}\right)\cdot6 H _{2} O }

When oxidised with \mathrm{KMnO_4}, only \mathrm{Fe^{2+}}will get oxidised to \mathrm{Fe^{3+}}

Thus, n-factor of Mohr's salt is 1.

Now, from law of equivalence, we have,

\mathrm{N_{1} V_{1}=N_{2} V_{2}}

Putting values ____

\mathrm{0.01 \times 5 \times v_{1}=0.05 \times 1 \times 20}

\mathrm{v_{1}=20\; \mathrm{ml}}

Thus 20 ml of \mathrm{KMnO_4} will be used in the titration.

Volume left =50-20=30\; \mathrm{ml}

Hence, 30 is answer

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