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Solution Preparation and Dilutions

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Presentation on theme: "Solution Preparation and Dilutions"— Presentation transcript:

1 Solution Preparation and Dilutions

2 Solution Preparation How do we create chemical solutions in a laboratory setting with a certain concentration/molarity? Obtain the mass of the chemical compound serving as solute Dissolve the solute in a small amount of the solvent Add enough solvent to reach the desired volume.

3 Example 1: Prepare a 6L solution of 4M NaCl 1392g NaCl

4 Example 2: Prepare a 250 ml solution of 0.05M HCl 0.45g HCl

5 Example 3: Prepare a 400 ml solution of 5M CuSO4 320g CuSO4

6 Dilutions

7 What is a dilution? Taking a CONCENTRATED solution and making it LESS concentrated Adding more solvent to decrease the amount of solute in the solution M1V1 = M2V2 Used when 2 solutions are involved Units do not matter but keep the same units throughout the problem !!! Ex. Tea and sweetner

8 Example 1: Prepare 2.50L of a 0.360M H2SO4 solution from a stock H2SO4 solution of 18.0 M. 50 ml of 18.0 M sulfuric acid

9 Example 2: A stock solution of KF has a concentration of 1.20M. To what final volume must 100ml of this solution be diluted to produce a 0.45 solution of KF? 0.267L, 267 ml

10 Example 3: What volume of 17.4 M acetic acid is needed to prepare 1.00 L of 3.00 M acetic acid? How much water would I need to add to 500ml of a 2.4M KCl solution to make a 1.0M solution? 0.172 L or 172 ml

11 Serial Dilutions A type of dilution
The dilution is made through a series of smaller dilutions from a stock or original solution Dilution factor Amount transferred/(amount transferred + amount of water) 1 ml of chemical solution into 9 ml of water is a 1/10 dilution factor. **How dilute is the resulting solution, multiply the dilution factors for each series.

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