. If 20.0 mL of a 0.10 M HCl solution is mixed with 10.0 mL of a 0.25 M HCl solution, what is the final concentration of HCl after the two solutions are mixed?
densty
Easiest is to multiply ml x M, add them and divide by total volume (30.0 ml).
An SI perfectionist would include a factor to divide ml/1000, but this is not needed as it appears all the way through.
If you post the answer I can check it.
To find the final concentration of HCl after mixing the two solutions, you need to apply the concept of dilution. The formula for dilution is:
C1V1 = C2V2
Where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume. In this case, we have:
C1 = 0.10 M (concentration of the first solution)
V1 = 20.0 mL (volume of the first solution)
C2 = ? (final concentration)
V2 = 20.0 mL + 10.0 mL = 30.0 mL (total volume after mixing)
By substituting these values into the formula, we can solve for the final concentration (C2):
(0.10 M)(20.0 mL) = C2(30.0 mL)
2.0 = C2(30.0 mL)
C2 = 2.0 / 30.0
C2 ≈ 0.067 M
Therefore, the final concentration of HCl after the two solutions are mixed is approximately 0.067 M.