1. Daily Science April 30
Determine if the following are soluble or insoluble
NaCl
HgS
LiOH
Will there be a precipitate in the following reaction?
NaCl + AgNO3 

2. Molarity
Pg. 111

3. Molarity Tells you the concentration of a solution M
The number of moles of solute dissolved per liter of solution
Read as molar
Must be in liters!

4. Calculating molarity M = moles of solute/ liters of solution
Unit= mol/L or M
Ex. What is the molarity of a solution containing 40.0 g of glucose (C6H12O6) in a 1.5 L solution?
Ex. What is the molarity of a bleach solution containing 9.5 g of NaOCl per 500 ml of bleach

5. Preparing solutions
If you know you need a certain molarity solution, you can calculate how many grams you need to measure out.
You first have to add the solute to a volumetric flask
Then you can fill the volumetric flask to the line with water
Can’t just add the volume of solvent you need because the solute takes up space
Ex. How many grams of CaCl2 would be dissolved in 1.0 L of a M solution of CaCl2?
Ex. How many grams of NaOH do you need to make a 1.5 L, 2.0 M solution of NaOH?

6. Diluting solutions Less concentrated solutions are diluted solutions
You can determine how much solvent you need to add to dilute a solution from a stock solution
M1V1 = M2V2
Ex. What volume of a M KI stock solution would you use to make L of a 1.25 M KI solution?
Ex. How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare mL of 0.25 M H2SO4?

7. Other Solutions
Electrolytic solutions- contain dissolved salts that can conduct electricity.
Heterogeneous solutions:
Colloids- intermediate molecules mixed in a dispersion medium (ex milk)
Suspensions- large particles mixed in a dispersion medium. Particles will settle or can be filtered out. (ex. Cornstarch and water)