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 =121.8g
and weight of 100 mL of H2SO4 solution (70%) =1.610×100 =161g Weight ofH2SO4(30%)=121.8×30100=36.54g Weight ofH2SO4(70%)=161×70100=112.7g
Total weight of H2SO4 (solute) =36.54+112.7=149.24 g Moles ofH2SO4=149.2498=1.5228 (molecular weight of H2SO4=98)