A chemist must dilute 99.9 mL of 161. mM aqueous silver perchlorate (AgClO,) solution until the concentration falls to 117. mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to 3 significant digits.

Introductory Chemistry: A Foundation
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A chemist must dilute 99.9 mL of 161. mM aqueous silver perchlorate (AgClio,) solution until the concentration falls to 117. mM. He'll do this by adding
distilled water to the solution until it reaches a certain final volume.
Calculate this final volume, in liters. Round your answer to 3 significant digits.
Transcribed Image Text:A chemist must dilute 99.9 mL of 161. mM aqueous silver perchlorate (AgClio,) solution until the concentration falls to 117. mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to 3 significant digits.
Expert Solution
Step 1

Dilution of the solution:

When we dilute a concentrated solution with pure water, the mole of solute remains constant in the initial solution and in the final solution. The mole of solute can be calculated by multiplying the molarity of the solution and the volume of the solution.

mole of solute=molarity of the solution×volume of the solution

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