1. Solubility ~A measure of how soluble something is.
Nothing is completely soluble or completely insoluble.
Increasing the temperature normally increases the amount of a solid solute a solution can hold.

2. Gases dissolved in a liquid
Colder solutions hold more of a gaseous solute.
Heating a solution forces gases to come out of solution (pre-boiling bubbles)
Higher pressure solutions can hold more gases.
~Why a pop can fizzes when opened

3. Decompression Sickness
If you dive deep into the ocean (submarine or scuba) the pressure increases
More gases will dissolve in the fluids of your body
If you rise too quickly, gases dissolved in the fluids of your body will come out of solution
This painful and deadly situation is called decompression sickness or “the bends”

4. Saturation
Saturated solution- solution that has all the solute it can hold. If any more is added it will not dissolve.
Supersaturated solution- a soln. holding more solute than it should
Made by heating a solution to dissolve more solute and then cooling it.
If you disturb a supersaturated solution the solute will fall out of solution.

5. Solubility Curve
Graph of grams of solute
vs. temperature
100 80 60 40 20
KNO3
KCl
g of solute
per 100 g
of water
NaCl
NH3
Temperature (oC)

6. Other units of concentration

7. Dilution Equation MV = MV Molarity (volume) before dilution
= molarity (volume) after dilution
How many liters of 12 M H2SO4 do you need to make 1.2 L of .75 M?
12 M (V) = .75 M (1.2 L)
V = .075 L (75 mL)

8. Mass Percent Mass percent = mass of solute x 100 mass of solution
Or = grams of solute x 100
grams of solute + grams of solvent

9. Problem
35 g of NaCl is dissolved in 115 g of water, what is the mass percent? What is the molarity if the final solution has a density of 1.1 g/mL?
35 g / (35g + 115g) x 100
23 %
35 g x 1 mol/ g= mol NaCl
150 g x 1mL / 1.1 g = mL = L
M = mol / L
M = 4.4 M

10. Convert
Convert 1.2 M CuSO4 solution to mass percent, if the solution has a density 1.1 g/mL.
1.2 M= 1.2 mol CuSO4 / 1 L solution
1.2 mol x g / 1 mol = g
1 L = 1000 mL x 1.1 g/1 mL = 1100 g of solution
Mass percent = g / 1100 g x100 = 17 %