Consider that you have a 100 mM stock solution and you need to prepare 10 mL of a 30 mM solution. How many milliliters of the stock solution do you need? mL How many milliliters of deionized water do you need? mL

Question

Chemistry

Gavyn Avery

2 July, 13:19

Consider that you have a 100 mM stock solution and you need to prepare 10 mL of a 30 mM solution. How many milliliters of the stock solution do you need? mL How many milliliters of deionized water do you need? mL

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Answers (1)

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Brooklynn Garrison · Answer 1

V₁ = 3.0 mL

V (H₂O) = 7 mL

Explanation:

Given data

Initial concentration (C₁) : 100 mM Initial volume (V₁) : ? Final concentration (C₂) : 30 mM Final volume (V₂) : 10 mL

In order to determine the volume of the stock solution, we will use the dilution rule.

C₁ * V₁ = C₂ * V₂

100 mM * V₁ = 30 mM * 10 mL

V₁ = 3.0 mL

The volume of deionized water required is:

V (H₂O) = 10 mL - 3.0 mL = 7 mL