Question

# Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and...

Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL. How much concentrated solution would you take to prepare 2.75 L of 0.460 M HCl by mixing with water?

To solve this problem we have to calculate the molarity of stock HCl solution. Then we can calculate the required volume of the concentrated solution to make a dilute solution.

37% HCl solution by mass means 37g of HCl are present in 100g of the solution

Volume of 100g of solution = mass / density = 100 / 1.2 = 83.33mL

In other words 37g of HCl is present in 83.33 mL of solution

37g of HCl = 37/36.5 = 1.013 moles of HCl., Because mlar mass of HCl = 36.5g

So 1.013 moles of HCl are present in 83.33mL of solution

Molarity = (No. of moles of solute / Volume of solution mL) X 1000

Molarity = (1.013 / 83.33) X 1000 = 12.1M

Use M1V1 = M2V2 equation to calculate the volume of concentrated solution to make dilute solution

M1 = 12.1M, V1 = ?, M2 = 0.460M, V2 = 2.75L

12.1M X V1 = 2.75 X 0.46M

V1 = 0.1045L = 104.5mL

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