Answer to Question #103257 in Chemistry for Chris

Question

a chemist must dilute 45.8 ml of 1.26 m aqueous barium acetate (Ba(C2H3O2)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.

Answer 1

The number of moles of barium acetate in the initial solution equals:

n = c₁ × V₁,

where n - number of moles, c₁ - molar concentration of the initial solution, V₁ - volume of the initial solution.

As number of moles is not changed after the dilution, volume of the final solution is:

V₂ = n / c₂,

where V₂ - volume of the final solution, c₂ - molar concentration of the final solution, n - number of moles.

As n = c₁ × V₁, than:

V₂ = c₁ × V₁ / c₂ = 1.26 M × 45.8 ml / 1.00 M = 57.7 ml

Answer: 57.7 ml