Analyze a situation involving the dilution of a solution in order to relate the number of moles, the volume and the molarity of the initial and the diluted solution.
Anna Litical obtains 0.110 L of a 2.150 M HCl(aq) stock solution. This volume is then diluted with distilled water to a final volume of 0.730 L.
How many moles of HCl are in 0.110 L of the stock solution?
# of Moles of HCl
mol
How many moles of HCl are in the final solution?
What is the molar concentration of the final solution?
Molarity
M
On Day 1 of a multi-day lab, lab partners Ray Ahn and Polly Ester prepare a 1.28 M aqueous solution of NaOH. On Day 2, Ray and Polly take 35.0 mL of this stock solution and dilute it with water to make a 140.0-mL solution.
How many moles of NaOH did Ray and Polly withdraw from the stock solution?
# of Moles of NaOH
What is the final concentration of this Day 2 solution?
Final Molarity
It is Acid-Base time and that means its time for Mrs. Stymone to make a batch of Barney’s Brew for all the Chemistry classes. She plans to make 2.80 L of 0.264 M HC2H3O2(aq) solution. She will do this by diluting a 5% by mass aqueous solution of HC2H3O2(aq) that has a density of 1.02 g/mL.
How many moles of HC2H3O2(aq) does Mrs. Stymone need in her final solution?
# of Moles of HC2H3O2
Use conversion factors to determine the volume of the 5% solution that Mrs. Stymone will need to use to make 2.80 L of 0.264 M HC2H3O2(aq) solution?
Volume of Solution
mL
What is the H2SO4 concentration of an aqueous solution prepared by diluting 30.0 mL of a 0.506 M H2SO4 solution to a final volume of 1.40 L?
[H2SO4] =
Anna Litical pipettes 25.00 mL of 2.97 M HCl into a 200.0-mL volumetric flask partly filled with distilled water. She then fills the flask with distilled water to the 200.0-mL mark. What is the final molar concentration of HCl?
[HCl] =
Mr. Glynch needs 750.0 mL of 1.10 M HCl solution for a lab. He will make the solution by diluting a concentrated solution of HCl. What volume of concentrated, 11.7 M HCl solution should he use?
Volume