How do you prepare 250.00 ml of 3.00 m hcl solution starting with a concentrated hcl solution which is 36.0% hcl by mass and has a density of 1.18 g/ml?

64.1 ml of concentrated is taken and (250-64.4)= 185.6 ml f water is added to make 250.00 mL of 3.00 M HCl .

Explanation:

Given : 36 g of is dissolved in 100 g of solution.

Density of solution = 1.18 g/ml

Thus volume of solution =

where,

n= moles of solute

= volume of solution

According to the dilution law,

where,

= molarity of stock solution = 11.7M

= volume of stock solution = V ml

= molarity of diluted solution = 3.00 M

= volume of diluted solution = 250.0 ml

Thus 64.1 ml of stock is taken and (250-64.4)= 185.6 ml of water is added to make 250.00 mL of 3.00 M HCl .

thats how its supposed to be