1. Drill:
What are the factors that determine how fast a substance dissolves?

2. Objective The student will be able to:
Explore concentrations of solutions in order separate food coloring dyes by paper chromatography.

3. SAT Enrichment
What is the pH of 0.05 M Mg(OH)2?
1.4
1.3
5.6
12.3
12.6

4. Concentrations of Solutions
What is Molarity??

5. Concentrations of Solutions
Water must be tested continually to ensure that the concentrations of contaminants do not exceed established limits. These contaminants include metals, pesticides, bacteria, and even the by-products of water treatment. You will learn how solution concentrations are calculated.

6. Molarity
The concentration of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent.
A dilute solution is one that contains a small amount of solute.
A concentrated solution contains a large amount of solute.

7. Molarity
Molarity (M) is the number of moles of solute dissolved in one liter of solution.
To calculate the molarity of a solution
The photos show how to make a 0.5-molar (0.5M) solution. a) Add 0.5 mol of solute to a 1-L volumetric flask half filled with distilled water. b) Swirl the flask carefully to dissolve the solute. c) Fill the flask with water exactly to the 1-L mark.

8. Molarity
To make a 0.5-molar (0.5M) solution, first add 0.5 mol of solute to a 1-L volumetric flask half filled with distilled water.

9. Molarity
Swirl the flask carefully to dissolve the solute.

10. Molarity
Fill the flask with water exactly to the 1-L mark.

11. Calculating Molarity

12. Calculating Molarity

13. Making Dilutions
Diluting a solution reduces the number of moles of solute per unit volume.
Total number of moles of solute in solution does not change.
M1 and V1 are the molarity and volume of the initial solution, and M2 and V2 are the molarity and volume of the diluted solution.

14. Making a Dilute Solution

15. Making Dilutions
To prepare 100 ml of 0.40M MgSO4 from a stock solution of 2.0M MgSO4, a student first measures 20 mL of the stock solution with a 20-mL pipet.
The student is preparing 100 mL of 0.40M MgSO4 from a stock solution of 2.0M MgSO4 . a) She measures 20 mL of the stock solution with a 20-mL pipet. b) She transfers the 20 mL to a 100-mL volumetric flask. c) She carefully adds water to the mark to make 100 mL of solution. Inferring How many significant figures does the new molarity have?

16. Making Dilutions
She then transfers the 20 mL to a 100-mL volumetric flask.

17. Making Dilutions
Finally she carefully adds water to the mark to make 100 mL of solution.

18. Volume-Measuring Devices
Volumetric Pipet
Buret
Graduated Cylinder
Volumetric Flask

19. Percent Solutions
The concentration of a solution in percent can be expressed in two ways:
as the ratio of the volume of the solute to the volume of the solution
as the ratio of the mass of the solute to the mass of the solution.

20. Percent Solutions
Concentration in Percent (Volume/Volume)

21. Percent Solutions
Isopropyl alcohol (2-propanol) is sold as a 91% solution. This solution consist of 91 mL of isopropyl alcohol mixed with enough water to make 100 mL of solution.
The label clearly distinguishes this solution of isopropyl alcohol from rubbing alcohol, which is a 70% solution of isopropyl alcohol. Applying Concepts How many milliliters of isopropyl alcohol are in 100 mL of 91% alcohol?

22. Percent Solutions
Concentration in Percent (Mass/Mass)

23. Quick Quiz
1. Diluting a solution does NOT change which of the following?
Concentration
volume
milliliters of solvent
moles of solute

24. Introduction to Chromatography
Purpose
To separate food coloring dyes by paper chromatography.
When finished complete the analysis questions and conclusion.
If you finish early complete “Going Further”.
Put your paper in the bin when finished!
40 min

25. Homework
Molarity Worksheet

26. Summary Did we accomplish the objective? Explain.
How do you calculate the molarity of a solution?
What is chromatography used for?
What were some observations you may have noticed about the different color food dyes? Explain.