The strengths of 5.6 volume hydrogen peroxide (of density 1 g/mL) in terms of mass percentage and molarity (M), respectively, are: (Take molar mass of hydrogen peroxide as 34 g/mol)
Solution
Volume strength = 11.2 × molarity
<br><br>$\Rightarrow$ molarity = ${{5.6} \over {11.2}}$ = 0.5
<br><br>Assuming 1 litre solution,
<br><br>mass of solution = 1000 ml × 1 g/ml = 1000 g
<br><br>mass of solute = moles × molar mass
<br><br>= 0.5 mol × 34 g/mol
<br><br>= 17 gm.
<br><br>$\therefore$ mass % = <span style="display: inline-block;vertical-align: middle;">
<div style="text-align: center;border-bottom: 1px solid black;">mass of solute</div>
<div style="text-align: center;">mass of solution</div>
</span> $\times$ 100
<br><br>= ${{17} \over {1000}} \times 100$ = 1.7 %
About this question
Subject: Chemistry · Chapter: Some Basic Concepts of Chemistry · Topic: Mole Concept
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