What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of
?

Question

What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of 
?

Quizplus · Accepted Answer

When diluting a solution, the initial and final amounts of solute must be equal. We can use the formula:

M1V1 = M2V2

where M1 = 12.0 M (initial concentration), V1 = 35.0 mL (initial volume), M2 = unknown final concentration, and V2 = 11.0 mL (final volume).

Solving for M2, we get:

M2 = (M1V1)/V2 = (12.0 M x 35.0 mL)/11.0 mL = 38.18 M/mL

We need to convert this concentration to M, which means dividing by 1000 to convert from millimoles to moles and dividing by the final volume (11.0 mL) to get the concentration:

M2 = 38.18 M/mL / 1000 mL/L / 11.0 mL = 0.350 M

Therefore, the final concentration after dilution is 0.350 M, which corresponds to choice (D).

What Is the Final Concentration of a Solution Prepared by Diluting