Question

A chemist wants to make 1.5 L of 0.5M HBr by diluting a 6.OM HBr solution. Hon many liters of that solution should be used?

Answer 1

Answer : The volume of HBr solution used should be, 0.125 L.

Explanation :

Formula used :

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of HBr solution.

$M_2\text{ and }V_2$ are the molarity and volume of diluted HBr solution.

We are given:

$M_1=0.5M\\V_1=1.5L\\M_2=6.0M\\V_2=?$

Putting values in above equation, we get:

$0.5M\times 1.5L=6.0M\times V_2$

$V_2=0.125L$

Therefore, the volume of HBr solution used should be, 0.125 L.