A chemist must dilute 58.00ml of 13.5 aqueous silver (II) oxide solution until the concentration falls to 5.00M. 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.

Question

Rodney Mason

Physics

26 February, 23:36

A chemist must dilute 58.00ml of 13.5 aqueous silver (II) oxide solution until the concentration falls to 5.00M. 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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Answers (1)

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Darby · Answer 1

The given solution of silver oxide = 58 ml of 13.5 M of silver oxide

When we increase its volume, its molar concentration becomes less. To calculate the concentration of diluted solution, we can apply the following relation.

S₁ V₁ = S₂ V₂.

S₁ is molar strength when volume is V₁. S₂ is molar strength when volume is V₂

Puting the given values in the formula above,

58 x 13.5 M = V₂ x 5

V₂ = 58 x 13.5 / 5

= 156.6 ml.

= 157 ml after rounding off.