Question
The volume of water that must be added to a mixture of 250 ml of 0.6 M HCl and 750 ml of 0.2 M HCl to obtain 0.25 M solution of HCl is
Answer: Option C
:
C
We can see that the number of moles of
HCl should remain constant, as per the law of conservation of mass.
Since we have molarity, we can calculate number of moles using,
No. of moles = Molarity × volume of solution
Initial Number of moles = 250 × 0.6 + 0.2 × 750
Final number of moles = 0.25 (250 + 750 + Vrequired) Equating, we get
Vrequired=0.6×250+0.2×7500.25−[1000]=200ml
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:
C
We can see that the number of moles of
HCl should remain constant, as per the law of conservation of mass.
Since we have molarity, we can calculate number of moles using,
No. of moles = Molarity × volume of solution
Initial Number of moles = 250 × 0.6 + 0.2 × 750
Final number of moles = 0.25 (250 + 750 + Vrequired) Equating, we get
Vrequired=0.6×250+0.2×7500.25−[1000]=200ml
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