A solution of H_2O_2 used for hair bleaching | vedclass

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(B) Molarity $(M)$ is defined as the number of moles of solute per liter of solution.Given:Mass of $H_2O_2 = 5.0 \ g$Volume of solution = $100 \ mL =

Vedclass · Accepted Answer

$1.5$

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(B) Molarity $(M)$ is defined as the number of moles of solute per liter of solution.Given:Mass of $H_2O_2 = 5.0 \ g$Volume of solution = $100 \ mL = 0.1 \ L$Molar mass of $H_2O_2 = 34 \ g/mol$Step $1$: Calculate the number of moles of $H_2O_2$.Moles = $\frac{	ext{Mass}}{	ext{Molar mass}} = \frac{5.0 \ g}{34 \ g/mol} \approx 0.147 \ mol$Step $2$: Calculate Molarity.$M = \frac{	ext{Moles of solute}}{	ext{Volume of solution in liters}} = \frac{0.147 \ mol}{0.1 \ L} = 1.47 \ M \approx 1.5 \ M$.Therefore,the correct option is $B$.

$A$ solution of $H_2O_2$ used for hair bleaching contains approximately $5.0 \ g$ of $H_2O_2$ per $100 \ mL$ of solution. If the molar mass of $H_2O_2$ is $34 \ g/mol$,what is the molarity of this solution?

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