A 5.0 mL solution of H 2 O 2 liberates 1.27 g of iodine from an acidified KI solution. The percentage strength of H 2 O 2 is

Question

A 5.0 mL solution of H 2 O 2 liberates 1.27 g of iodine from an acidified KI solution. The percentage strength of H 2 O 2 is (A) 11.2 (B) 5.6 (C) 1.7 (D) 3.4

Tardigrade Admin · Accepted Answer

H 2 O 2 ≡ I 2 2 KI + H 2 O 2+ H 2 SO 4 arrow K 2 SO 4+2 H 2 O + I 2 mEq of H 2 O 2=5 × N mEq of 2=( text Weight / text E.w ) × 1000 (1.27/127) × 1000=10 mEq ∴ mEq of H 2 O 2= mEq of I 2 5 × N =10 ∴ N =2 1 N of H 2 O 2=1.7 % of H 2 O 2 2 N of H 2 O 2=3.4 % H 2 O 2

Q. A $5.0 m L$ solution of $H_{2} O_{2}$ liberates $1.27 g$ of iodine from an acidified $K I$ solution. The percentage strength of $H_{2} O_{2}$ is

$11.2$

$5.6$

$1.7$

$3.4$

Q. A 5.0mL solution of H2​O2​ liberates 1.27g of iodine from an acidified KI solution. The percentage strength of H2​O2​ is

11.2

5.6

1.7

3.4

H2​O2​≡I2​ 2KI+H2​O2​+H2​SO4​→K2​SO4​+2H2​O+I2​ mEq of H2​O2​=5×N mEqof2​= E.w Weight ​×1000 1271.27​×1000=10mEq∴mEq of H2​O2​=mEq of I2​ 5×N=10∴N=2 1N of H2​O2​=1.7% of H2​O2​ 2N of H2​O2​=3.4%H2​O2​

Q. A $5.0 m L$ solution of $H_{2} O_{2}$ liberates $1.27 g$ of iodine from an acidified $K I$ solution. The percentage strength of $H_{2} O_{2}$ is

$11.2$

$5.6$

$1.7$

$3.4$