1. When talking about a liquid-what does the word “solution” mean?

2.  A homogeneous mixture of two or more substances in a single physical state  Liquid  Solid  Gas

3. Solutions are homogeneous mixtures

4. A solute is the dissolved substance in a solution. A solvent is the dissolving medium in a solution. Solvent Salt in salt waterSugar in soda drinks Carbon dioxide in soda drinks Water in salt waterWater in soda

5.  Solubility can apply to different states of matter. Ability to dissolve.  Soluble – a substance that is able to dissolve in another substance.  Sugar in water  Salt in water  Insoluble – A substance that does not dissolve in another substance.  Oil in water

6.  Solid solutions  Alloys – two or more metals  Gaseous solutions  Air  Liquid solutions  Oxygen in water  Vinegar (acetic acid in water)  Aqueous solutions  Ions in water

7. Fats Benzene Steroids Hexane Waxes Toluene Polar and ionic solutes dissolve best in polar solvents Nonpolar solutes dissolve best in nonpolar solvents Inorganic Salts Water Sugars Small alcohols Acetic acid

8. Solids tend to dissolve best when: o Heated o Stirred o Ground into small particles Liquids tend to dissolve best when: o The solution is cold o Pressure is high

9.  A solution that contains the maximum amount of solute that may be dissolved under existing conditions is saturated.  A solution that contains less solute than a saturated solution under existing conditions is unsaturated.  A solution that contains more dissolved solute than a saturated solution under the same conditions is supersaturated.

10.  Do the following in your notebooks:  15-1 Section Review questions  #1-4, pg. 505  On pg. 532 do the “Concept Mapping” activity

11. What is a solute and what is a solvent?

12.  The concentration of a solution is the amount of solute in a given amount of solvent or solution.

13. Molarity - the ratio of moles of solute to liters of solution Molarity=M= moles of solute Liters of solution

14.  You need to be able to calculate molarity  Example:  What is the molarity of a solution formed by mixing 10.0g H 2 SO 4 with enough water to make 100.0mL of solution?  To solve:  Moles of solute? ▪ 10.o g H 2 SO 4  Liters of solution? ▪ 100.0mL

15.  How do we solve it?  convert our units  Divide solute by solution’s total volume  mL  L  Grams  moles 10.0g H2SO4 1mol H2SO4  Answer 1.02 M 0.100 L solution 98.1 g H2SO4 x

16.  Practice #1  Vinegar is a solution of acetic acid. What is the molarity of the solution when 125 g of acetic acid (C2H4O2) is dissolved in enough water to make 1.50 L of solution?  Answer  1.39M

17.  Practice #2  How many grams of bromine are needed to prepare 0.500 L of a 0.0100 M solution of bromine in water?  Answer  0.799 g

18.  To learn more about molarity and how to calculate it we will be doing a lab!  Beer’s Law (named after a person, not a beverage) states that you can determine the concentration of a solution by how much light it absorbs.  So, you will be making solutions of different concentrations and testing them

19.  Important to remember  Your measurements and calculations must be exact!  If you do not measure right, you will ruin your solution and you will have to begin again  You will do a graph-this MUST be done on graph paper or by computer-NO exceptions

20. Mole fraction – the ratio of moles of solute to total moles of solution

21. Calculate the Molarity of 98 grams of sodium hydroxide in 2.2 liters of solution.

22.  Getting started:  Create a data table  Make up your solution  This is from the calculations you made yesterday  50 mL total  You will use this to create all the dilutions  T0 make your dilutions:  M1V1=M2V2

23.  After you create the dilutions you will place a sample of your solution in the colorimeter  You will graph your results-on graph paper