100mL of an H2SO4 solution that has a molarity of 1M and density of 1.50 g/mL is mixed with 400mL of water. If the final density of the resulting solution is 1.25 g/mL, the final molarity of the H2SO4 solution is:
A
4.40M
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B
0.145M
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C
0.520M
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D
0.227M
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Solution
The correct option is D0.227M No. of moles of H2SO4 reacted = molarity x volume
= 1 M x 100mL
= 0.1 moles
Weight of H2SO4 = density x volume
=1.50 x 100 = 150 g
Weight of water reacted with H2SO4=400g
Total mass of the resulting solutionH2SO4=150+400g=550g
Total volume of the resulting solutionH2SO4=5501.25=440mL
Molarity =no.ofmolesvolume=0.1440×1000=0.227M