In the redox reaction, $2 {KMnO}_{4} + 3 H_{2} {SO}_{4} + 5 H_{2} C_{2} O_{4} \to$ $K_{2} {SO}_{4} + 2 {MnSO}_{4} + 10 {CO}_{2} + 8 H_{2} O,$
the volume of $0.1 M {KMnO}_{4}$ required to oxidize 25ml of $0.25 M H_{2} C_{2} O_{4}$ solution is.

see full answer

21% of IItians & 23% of AIIMS delhi doctors are from Sri Chaitanya institute !!

An Intiative by Sri Chaitanya

1.2. lit

25 lit

$125 ml$

$25 ml$

answer is C.

(Unlock A.I Detailed Solution for FREE)

Ready to Test Your Skills?

Check your Performance Today with our Free Mock Test used by Toppers!

Take Free Test

Detailed Solution

The provided reaction is:

$5 H_{2} C_{2} O_{4} + 2 {KMnO}_{4} + 3 H_{2} {SO}_{4} \to 2 {MnSO}_{4} + K_{2} {SO}_{4} + 10 {CO}_{2} + 8 H_{2} O$

According to the molarity equation

${(\frac{M_{1} V_{1}}{n_{1}})}_{K M n O_{4}} = {(\frac{M_{2} V_{2}}{n_{2}})}_{oxalic acid}$

or $\frac{0.1 \times V_{1}}{2} = \frac{0.25 \times 25}{5}$

$V_{1} = \frac{2 \times 0.25 \times 25}{5 \times 0.1} = \frac{12.5}{0.5}$

$V_{1} = 25 ml$

Hence, option(c) is the answer.

Watch 3-min video & get full concept clarity