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Diluting a Solution

Learn how to dilute concentrated solutions to the required concentration for experiments. Understand the relationship between initial and final solution volumes and concentrations. Examples provided for better understanding.

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Diluting a Solution

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  1. Diluting a Solution • Most solutions are stored in concentrated form and diluted for use when required. • To dilute to the required concentration we must extract the number of moles required from the stock solution and place them in the new flask. • Fill it with water and we are done

  2. The number of moles does not change when you dilute the solution, therefore: • Since n = Cv in both beakers, we can write the relationship as : • Civi = CfvfCi = Concentration of the initial solutionvi = volume of the initial solutionCf = Concentration of the final solutionvf = volume of the final solution

  3. EXAMPLE 1 • What volume of 12.4 mol/L hydrochloric acid is required to prepare 2.00 L of 0.250 mol/L solution.- note: whenever you want to prepare something, this will be a final concentration or volume

  4. ANSWER • Civi = Cfvf • 12.4 M (v) = 2.00 L x 0.250 M • v= (2.00L) x (0.250M/12.4M) • v = 0.0403 L or 40.3 mL

  5. EXAMPLE 2 • What is the concentration of the diluted acetic acid if 200 mL of 17.4 M is pipette into a 500 mL flask and brought up to the full volume?

  6. ANSWER #2 • Civi = Cfvf (note:200mL=0.200L) • 17.4 M x 0.200 L = Cf x 0.500 L • Cf = 6.96 M

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