1. ACT Prep Passage II 5 minutes Start when the bell rings
WARM UP
ACT Prep
Passage II
5 minutes
Start when the bell rings

2. Solubility Factors

3. Solution Terms
Insoluble
Won’t dissolve
Soluble
Will dissolve

4. Why did the white bear dissolve in water? Because it was a polar bear.
IMF and Solubility
“Like dissolves like”
Similar IMF will dissolve
Polar = polar/ionic Nonpolar = nonpolar
Chemistry Humor
Why did the white bear dissolve in water? Because it was a polar bear.

5. Nitrates (NO3-), bicarbonates (HCO3-), and chlorates (ClO3-)
IMF and Solubility
Exception: Some ionic compounds in water (Table 4.2)
Soluble
Exceptions
Compounds containing alkali metal ions (Li+, Na+, K+, Rb+, Cs+) and the ammonium ion (NH4+)
Nitrates (NO3-), bicarbonates (HCO3-), and chlorates (ClO3-)
Halides (Cl-, Br-, I-)
Halides of Ag+, Hg22+, and Pb2+
Sulfates (SO42-)
Sulfates of Ag+, Ca2+, Sr2+, Ba2+, Hg22+, and Pb2+
Insoluble
Exceptions
Carbonates (CO32-), phosphates (PO43-), chromates (CrO42-), and sulfides (S2-)
Compounds containing alkali metal ions and the ammonium ion
Hydroxides (OH-)
Hydroxides containing alkali metal ions and the Ba2+ ion

6. Temperature and Solubility
Solids
Increases with increasing temperature
Examples
Kool-Aid in the fridge

7. Temperature and Solubility
Gases
Decreases with increasing temperature
Examples
Pre-boil bubbles
“Flat” pop

8. Pressure and Solubility
Gases are more soluble with increasing pressure
Henry’s Law (William Henry)
Examples
Pop “fizz”

9. WRAP UP
Use Table 4.2 to determine the solubility (in water) of each of the following:
KOH Ca3(PO4)2
NaCl AgNO3