A 5.0 cm3 solution of H2O2 liberates 0.508 g of iodine from an acidified KI solution. Calculate the strength of H2O2 solution in terms of volume strength at STP.

Question

A 5.0 cm3 solution of H2O2 liberates 0.508 g of iodine from an acidified KI solution. Calculate the strength of H2O2 solution in terms of volume strength at STP. (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

The redox reaction involved is H2O2 +2I- +2H+ arrow 2H2 O +I2 If M is molarity of H2 O2 solution, then 5M =(0.508 × 1000/254)(∵ 1 mole H2O2 ≡ 1 mole I2) ⇒ M=0.4 Also, n-factor of H2O2, is 2, therefore normality of H2O2 , solution is 0.8 N. ⇒ Volume strength = Normality × 5.6 = 0.8 × 5.6 = 4.48 V

Q. A 5.0cm3 solution of H2​O2​ liberates 0.508g of iodine from an acidified KI solution. Calculate the strength of H2​O2​ solution in terms of volume strength at STP.

Q. A $5.0 c m^{3}$ solution of $H_{2} O_{2}$ liberates $0.508 g$ of iodine from an acidified $K I$ solution. Calculate the strength of $H_{2} O_{2}$ solution in terms of volume strength at STP.