A chemist must dilute 75.4 mL of 1.17 M aqueous barium acetate (Ba(C_2H_2O_2)_2) solution until the concentration falls to 1.00 M. He'll do this by adding distilled water to the solution until it reaches a certain final volume
Calculate this final volume, in milliliters. Round your answer to 3 significant digits.
To dilute the solution, we can use the formula:
M1V1 = M2V2
Where:
M1 = initial concentration of barium acetate solution = 1.17 M
V1 = initial volume of barium acetate solution = 75.4 mL
M2 = final concentration of barium acetate solution = 1.00 M
V2 = final volume of diluted solution (which we need to calculate)
Plugging in the values, we get:
(1.17 M)(75.4 mL) = (1.00 M)(V2)
89.118 = 1.00(V2)
V2 = 89.118 mL
Therefore, the chemist must add distilled water to the barium acetate solution until the final volume reaches 89.118 mL. Rounded to 3 significant digits, the final volume would be 89.1 mL.