Problem: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.95 L of an HCl solution with a pH of 1.8?

FREE Expert Solution

We have to determine the volume of 36.0 % by mass HCl solution required to prepare 4.95 L of a solution with a pH of 1.8.


Recall: halogen binary acids are strong acids, except HF.

HCl is a strong acid and dissociates completely in solution.

HCl → H+ + Cl-


We will solve this problem through these steps:

Step 1: Calculate the concentration of final solution using the given pH.

Step 2: Calculate the molarity of 36.0 % by mass HCl solution (stock solution).

Step 3: Use the dilution formula and calculate the required volume.

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Problem Details

What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.95 L of an HCl solution with a pH of 1.8?

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Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.