A chemist must dilute 57.6 ml of 1.41 M aqueous barium acetate (Ba(C,H,02), 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 mililiters. Be sure your answer has the correct number of significant digit mL
The equation for dilution calculations can be used.
c1, V1 - the molarity and volume of the concentrated solution
c2, V2 - the molarity and volume of the diluted solution
(1.41 M) × (57.6 mL) = (1.00 M) × V2
V2 = (1.41 M × 57.6 mL) / (1.00 M) = 81.216 mL = 81.2 mL
V2 = 81.2 mL
Answer: The final volume is 81.2 mL.