1. Solutions
To play the movies and simulations included, view the presentation in Slide Show Mode.

2. I stored sodas in a small refrigerator
I stored sodas in a small refrigerator. One day I noticed that the Diet Coke had exploded from freezing but the regular Coke did not freeze and therefore did not explode.
I thought why did the Diet Coke freeze and not regular Coke?
Regular coke has about 39 grams of sugar dissolved in it.
The 39 grams of sugar interfered with the water trying to freeze. So the freezing point of regular Coke was lower than that of Diet Coke.

3. Definitions
A solution is a mixture of 2 or more substances in a single phase.
solute + solvent=> solution

4. Parts of a Solution
SOLUTE – the part of a solution that is being dissolved (less amount)
SOLVENT – the part of a solution that dissolves the solute ( greater amount)
Solute
Solvent
Example
solid
liquid
gas

5. Concentration of a Solution
The amount of solute in a solution is given by its concentration, or molarity
M = n / V and n = m / MM
Molarity ( M ) =
moles solute
liters of solution

6. PROBLEM: Dissolve 5.00 g of NiCl2 in enough water to make 250 mL of solution. Calculate the Molarity.
Step 1: Calculate moles of NiCl2
Step 2: Calculate Molarity

7. USING MOLARITY What mass of oxalic acid, H2C2O4, is
required to make 580 mL of a M
solution?
1.13 g

8. Percent Solutions Density = mass / volume d H2O = 1g/ mL
1. Volume/Volume
When both solute and solvents are liquids.
Percent by volume( % v/v) = volume of solute x 100%
______________
volume of solution

9. What is the percent by volume of ethanol in the final solution when 85mL of ethanol is diluted with 250 mL of water?
85/300 x 100 = 28.3%

10. A bottle of the antiseptic hydrogen peroxide, H2O2 is labeled 3
A bottle of the antiseptic hydrogen peroxide, H2O2 is labeled 3.0 %(v/v). How many mL of hydrogen peroxide are in a 2 L bottle of this solution?
What is the molarity?

11. When both solute and solvent are solids.
2. Mass / Mass
When both solute and solvent are solids.
Percent by mass( % m/m) = mass of solute x 100%
______________
mass of solution
How many grams of potassium sulfate are required to make 1500g of a 5% m/m solution?
How much water?
75g of solute dissolved in 1425g of water, page 486

12. 3. Mass/ Volume ( % m/v) Percent ( % m/v) = mass of solute x 100%
_____________
volume of solution
18 g of ethanol dissolves in 400 mL of water. What is the concentration in % m/v ?

13. Making Dilutions M1 V1 = M2 V2
Where: M1 = concentration of the first solution V1 = volume of the first solution M2 = concentration of the second solution V2 = volume of the second solution
Examples:
1.How many mililiters of a solution of 4M KI are needed to prepare 400 mL of a 0.76 M ?
2. How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?
Add nnugh water up to becoe2.5 L

14. 3) How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?
4) I have 345 mL of a 1.5 M NaCl solution. If 100 mL of water evaporates, what will the molarity of the solution be?

15. If I add 15g of CaCl2 to a flask and complete to a final volume of 500 mL,
A) What is the % by mass?
B) What is the molarity of the solution?

16. Question 12
If I make a solution by adding water to 35 mL of methanol until the final volume of the solution is 275 mL…
a) What is the molarity of methanol in this solution? (The density ofmethanol is g/mL)

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