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Question

100 mL of an H2SO4 solution that has a molarity of 1 M and density of 1.50 g/mL is mixed with 400 mL of water. If the final density of the resulting solution is 1.25 g/mL, the final molarity of the H2SO4 solution is:

A
4.40 M
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B
0.145 M
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C
0.520 M
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D
0.227 M
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Solution

The correct option is D 0.227 M
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. of molesvolume=0.1440×1000=0.227M

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