The concentration of an oxalic acid solution is x `mol` `litre^-1`. `40mL` of this solution reacts with `16mL` of `0.05M` acidified `KMnO_4`. What is the `pH` of 'x' M oxalic acid solution ? (Assume that oxalic acid dissociates completely).)

Options

A. `1.3`
B. `1.699`
C. 1
D. 2

Answer

C

Explanation

for any redox reaction `(M_(1)V_(1))/(n_(1))=(M_(2)V_(2))/(n_(2))` 2 moles `KMnO_(4)` completed oxidised by `(0.05xx16)/(2)xx=(xxx40)/(5) " " 0.05M`
Normality of Oxalic acid `=0.05 x 2=0.1`
`[H^(+)]=10^(-1) " " P^(H)=1`