Question:

A solution of H2SO4 \text{H}_2\text{SO}_4 is 31.4% H2SO4 \text{H}_2\text{SO}_4 by mass and has a density of 1.25g/mL 1.25 \, \text{g/mL} . The molarity of the H2SO4 \text{H}_2\text{SO}_4 solution is _____ M (nearest integer).
[Given molar mass of H2SO4=98g/mol \text{H}_2\text{SO}_4 = 98 \, \text{g/mol} ]

Updated On: Nov 13, 2024
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Correct Answer: 4

Solution and Explanation

To find the molarity (M), use the formula:

M=nsoluteV×1000 M = \frac{n_{\text{solute}}}{V} \times 1000

Given that the solution is 31.4% H2SO4 H_2SO_4 , with a density of 1.25 g/mL:

Step 1: Calculate the mass of H2SO4 H_2SO_4 in 100 g of solution:

Mass of H2SO4=31.4g H_2SO_4 = 31.4 \, \text{g}

Step 2: Convert this to moles:

31.498=0.32mol \frac{31.4}{98} = 0.32 \, \text{mol}

Step 3: Find the volume of the solution:

Volume=Mass of solutionDensity=1001.25=80mL \text{Volume} = \frac{\text{Mass of solution}}{\text{Density}} = \frac{100}{1.25} = 80 \, \text{mL}

Step 4: Calculate molarity:

M=0.32mol80mL×1000=4.0054M M = \frac{0.32 \, \text{mol}}{80 \, \text{mL}} \times 1000 = 4.005 \approx 4 \, \text{M}

So, the correct answer is: 4M

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