What is the amount of H_2O_2 in grams present | vedclass

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(B) The normality $(N)$ of a solution is given by the formula: $N = \frac{	ext{Mass in grams}}{	ext{Equivalent weight} 	imes 	ext{Volume in Liters

Vedclass · Accepted Answer

$25.5$

Vedclass · Answer

(B) The normality $(N)$ of a solution is given by the formula: $N = \frac{	ext{Mass in grams}}{	ext{Equivalent weight} 	imes 	ext{Volume in Liters}}$.For $H_2O_2$,the molar mass is $34 \ g/mol$. Since the $n$-factor for $H_2O_2$ in redox reactions is $2$,the equivalent weight is $\frac{34}{2} = 17 \ g/eq$.Given $N = 1.5 \ N$ and $V = 1 \ L$,we have: $1.5 = \frac{	ext{Mass}}{17 	imes 1}$.Therefore,$	ext{Mass} = 1.5 	imes 17 = 25.5 \ g$.

What is the amount of $H_2O_2$ in grams present in $1 \ L$ of $1.5 \ N$ $H_2O_2$ solution?

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