A chemist must dilute 34.3mL of 1.72mM aqueous calcium sulfate solution until the concentration falls to 1.00mM. 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.

Often times, the concentration of a standard solution may have to be diluted to a lower one by adding distilled water. To find the find the final volume, we must recognize that the number of moles of the substance in initial and final solutions are the same.

Therefore;

C₁V₁ = C₂V₂

where C and V are concentration and 1 and 2 are initial and final states.

now input the variables;

1.72 x 10⁻³ x 0.0343 = 1 x 10⁻³ x V₂

V₂ = 0.0589dm³ = 58.9mL

A chemist must dilute 34.3mL of 1.72mM aqueous calcium sulfate solution until the concentration falls to 1.00mM. 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.

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A chemist must dilute 34.3mL of 1.72mM aqueous calcium sulfate solution until the concentration falls to 1.00mM. 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.