Question

Calculate the volume of 0.015M HCL solution required to prepare 250 ml of a 5.25×10*3 M HCL solution

Answer 1

M1 = 0.015 mol/L

M2 = 5.25 X 10^3 mol/L

V2 = 250ml

Moles of HCl will be same in both cases,

M1V1 = M2V2

0.015 x V1 = 5.25 x 10^3 x 250

V1 = 87500L

Answer 2

The volume of diluted solution of HCl is $8.75\times 10^7mL$

Explanation:

To calculate the molarity of the diluted solution, we use the equation:

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of the concentrated HCl solution

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

We are given:

$M_1=5.25\times 10^3M\\V_1=250mL\\M_2=0.015M\\V_2=?mL$

Putting values in above equation, we get:

$5.25\times 10^3\times 250.0=0.015\times V_2\\\\V_2=\frac{5.25\times 10^3\times 250}{0.015}=8.75\times 10^7mL$

Learn more about dilution law:

https://brainly.com/question/14588135

https://brainly.com/question/3459109

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