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Question

A solution is made by mixing equal volumes of 30% by weight of H2SO4 (density = 1.218 g/mL) and 70% by weight of H2SO4 (density = 1.610 g/mL). Then find the molarity of the final solution?

A
11.4 M
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B
7.6 M
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C
3.6 M
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D
5.5 M
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Solution

The correct option is B 7.6 M
Suppose that the solution contains 100 mL of each variety of H2SO4. Total volume is, therefore, 200 mL or 0.2 L
Weight of 100 mL of H2SO4 solution (30%)=1.218×100
=121.8 g
and weight of 100 mL of H2SO4 solution (70%)
=1.610×100
=161 g
Weight of H2SO4 (30%)=121.8×30100=36.54g
Weight of H2SO4(70%)=161×70100=112.7 g
Total weight of H2SO4 (solute)
=36.54+112.7=149.24 g
Moles of H2SO4=149.2498=1.5228 (molecular weight of H2SO4=98)

Molarity=1.52280.2=7.6 M

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