Question

What volume of concentrated hydrochloric acid (12.0 M HCl) is required to make 2.0 liters of a 3.0 M HCl solution?
A) 5.0 liters
B) 0.24 liters
C) 0.50 liters
D) 6.0 liters

Answer 1

For the answer to the question above asking what volume of concentrated hydrochloric acid (12.0 M HCl) is required to make 2.0 liters of a 3.0 M HCl solution? The answer is 3.0/12.0 * 2 L = So it's  C

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Answer 2

Answer : The correct option is, (C) 0.50 liters

Solution :

According to the neutralization law,

$M_1V_1=M_2V_2$

where,

$M_1$ = molarity of concentrated HCl solution = 12.0 M

$V_1$ = volume of concentrated HCl solution = ?

$M_2$ = molarity of HCl solution = 3.0 M

$V_2$ = volume of HCl solution = 2.0 L

Now put all the given values in the above law, we get the volume of concentrated HCl solution.

$(12.0M)\times V_1=(3.0M)\times (2.0L)$

$V_1=0.50L$

Therefore, the volume of 12.0 M concentrated HCl required will be, 0.50 liters.