Question

A 28.9 mL aliquot of a 3.2 M Hal stock solution is diluted to a 454.0 mL of solution. What is the HCl concentration of the diluted solution

a.) 4.9 M
b.) .093 M
c.) .2 M
d.) .5 M

Answer 1

The final concentration of HCl after dilution is approximately 0.204 M, which we round to 0.20 M due to significant figures.

Step-by-step explanation:

To determine the final concentration of the diluted HCl solution, we need to use the concept of dilution of concentrated solutions. The formula for calculating the final concentration after dilution is:

(stock concentration) × (volume of aliquot) / (final volume) = final concentration

Plugging in the values provided:

((3.2 M) × (28.9 mL)) / (454.0 mL) = final concentration

We first need to convert mL to L to ensure consistent units. So, 28.9 mL is 0.0289 L and 454.0 mL is 0.454 L.

((3.2 M) × (0.0289 L)) / (0.454 L) = final concentration

Carry out the multiplication and division to find the final concentration:

(0.09248 M) / (0.454 L) ≈ 0.204 M

Therefore, the final concentration of the diluted HCl solution is approximately 0.204 M, which we would round to 0.20 M to reflect the significant figures from the initial concentration.