Hydrogen peroxide solution (20 ml) reacts quantitatively with a solution of KMn O 4 (20 ml) acidified with dilute H 2 S O 4 . The same volume of the KMn O 4 solution is just decolourized by 10

Question

Hydrogen peroxide solution (20 ml) reacts quantitatively with a solution of $KMn O_{4}$ (20 ml) acidified with dilute $H_{2} S O_{4}$ . The same volume of the $KMn O_{4}$ solution is just decolourized by 10 ml of $MnS O_{4}$ in neutral medium simultaneously forming a dark brown precipitate of hydrated $Mn O_{2}$ . The brown precipitate is dissolved in 10 ml of 0.1 M sodium oxalate under boiling condition in the presence of dilute $H_{2} S O_{4}$ . The strength of $H_{2} O_{2}$ solution in mg per 100 ml solution is

Answer:

170.00

Solution:

Oxalate = $10 \times 0.1$ = 1 mmol, so $Mn O_{2}$ = 1 mmol. $Mn O_{4}^{-}$ = 1×2/5 = 0.4 mmol in 20 ml ( $KMn O_{4}$ = 0.02 M). $H_{2} O_{2}$ = 0.4×5/2 = 1.0 mmol in 20 ml = 5 mmol per 100 ml = $5 \times 34$ = 170 mg/100 ml. Ans 0170.

TestHub · Accepted Answer

Oxalate = 10 × 0.1 = 1 mmol, so Mn O 2 ​ = 1 mmol. Mn O 4 − ​ = 1×2/5 = 0.4 mmol in 20 ml ( KMn O 4 ​ = 0.02 M). H 2 ​ O 2 ​ = 0.4×5/2 = 1.0 mmol in 20 ml = 5 mmol per 100 ml = 5 × 34 = 170 mg/100 ml. Ans 0170.

Chemistry - Redox Reactions Question with Solution | TestHub

Doubts & Discussion