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

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)* V_1=(3.0M)* (2.0L)`

`V_1=0.50L`

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

Answer 2

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

I hope my answer helped you. Feel free to ask more questions. Have a nice day!