What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a...

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Chemistry

What volume of a concentrated HCl solution, which is 36.0% HClby mass and has a density of 1.179 g/mL, should be used to make4.95 L of an HCl solution with a pH of 1.9?

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3.9 Ratings (602 Votes)

Required pH is 1.9
then using formula [H+] = 1^(-pH)

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â [H+] = 10^-1.90
Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â [H+] = 0.0125 mol / L

As HCl is a strong acid it dissociates completely, giving [H+] = [HCl]

In 4.95L solution we require 4.95*0.0125 = 0.0618 mol HCl

Molar mass HCl = 36.46 g/mol

0.0618 mol HCl = 0.0618*36.46 = 2.2532 g HCl

Our stock solution is 36.0% by mass that means 100g solution contains 36.0g HCl.

Mass of solution that contains 2.2532 g HCl = 2.2532/36.0*100 = 6.258 g HCl stock solution.

Volume of stock solution = mass / density
Volume = 6.258/1.179
Volume = 5.307 mL of the stock HCl solution required.

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