Question

Commercial HCl has a concentration of 12.1 M. What volume of commercial HCl should be used to make 250 mL of a 3.00 M HCl solution?

Answer 1

Approximately 62 mL of commercial HCl with a concentration of 12.1 M is needed to prepare 250 mL of a 3.00 M HCl solution, using the dilution formula M1V1 = M2V2.

Step-by-step explanation:

The question asks what volume of commercial HCl with a concentration of 12.1 M should be used to prepare 250 mL of a 3.00 M HCl solution.

To solve this, we can use the dilution formula M1V1 = M2V2, where:

• M1 is the molarity of the concentrated solution (12.1 M)
• V1 is the volume of the concentrated solution we want to find
• M2 is the molarity of the diluted solution (3.00 M)
• V2 is the volume of the diluted solution (250 mL)

Rearranging the formula to solve for V1, we get:

V1 = M2V2 / M1

Substituting the known values:

V1 = (3.00 M * 250 mL) / 12.1 M

V1 = (750 mL) / 12.1

V1 = 61.9835 mL

So, approximately 62 mL of the commercial HCl is needed to prepare 250 mL of a 3.00 M HCl solution.