1. Concentration Molarity Parts per Million Percent by Mass
Percent by Volume

2. Molarity
What is the molarity of a mL solution of NaOH (FM = 40.0) with 60.0 g of NaOH (aq)?
Convert g to moles and mL to L first!
M = moles / L = 1.50 moles / L = 3.00 M
How many grams of NaOH does it take to make 2.0 L of a M solution of NaOH (aq)?
Moles = M X L = M X 2.0 L = moles
Convert moles to grams: moles X 40.0 g/mol = 8.00 g

3. Parts Per Million
100.0 grams of water is evaporated and analyzed for lead grams of lead ions are found. What is the concentration of the lead, in parts per million?
ppm = ( g) / (100.0 g) X = 1.0 ppm
If the legal limit for lead in the water is 3.0 ppm, then the water sample is within the legal limits (it’s OK!)

4. Percent by Mass
A 50.0 gram sample of a solution is evaporated and found to contain grams of sodium chloride. What is the percent by mass of sodium chloride in the solution?
% Comp = (0.100 g) / (50.0 g) X 100 = 0.200%

5. Percent By Volume
Substitute “volume” for “mass” in the above equation.
What is the percent by volume of hexane if 20.0 mL of hexane are dissolved in benzene to a total volume of 80.0 mL?
% Comp = (20.0 mL) / (80.0 mL) X100 = 25.0%

6. Colligative Properties
Vapor Pressure Lowering
B.P. Elevation DTf= m. kf (or D Tb= m. kb)
F.P. Depression
Osmotic Pressure
Colligative properties depend upon # of particles (ions, atoms, molecule= particle)
Which will have lowest B.P. 1M NaCl, 1 M C6H12O6 or 1M Na3PO4?

7. Neutralization
10.0 mL of 0.20 M HCl is neutralized by 40.0 mL of NaOH. What is the concentration of the NaOH?
#H MaVa = #OH MbVb, so Mb = #H MaVa / #OH Vb
= (1)(0.20 M)(10.0 mL) / (1) (40.0 mL) = M
How many mL of 2.00 M H2SO4 are needed to completely neutralize 30.0 mL of M KOH?

8. Formulas, Naming and Properties of Acids
Arrhenius Definition of Acids: molecules that dissolve in water to produce H3O+ (hydronium) as the only positively charged ion in solution.
HCl (g) + H2O (l)  H3O+ (aq) + Cl-
Properties of Acids
Naming of Acids
Formula Writing of Acids

9. Properties of Acids
Acids react with metals above H2 on Table J to form H2(g) and a salt.
Acids have a pH of less than 7.
Dilute solutions of acids taste sour.
Acids turn phenolphthalein CLEAR, litmus RED and bromthymol blue YELLOW.
Acids neutralize bases.
Acids are formed when acid anhydrides (NO2, SO2, CO2) react with water for form acids. This is how acid rain forms from auto and industrial emissions.

10. Naming of Acids (polyatomic ion) -ate +ic acid
Binary Acids (H+ and a nonmetal)
hydro (nonmetal) -ide + ic acid
HCl (aq) = hydrochloric acid
Ternary Acids (H+ and a polyatomic ion)
(polyatomic ion) -ate +ic acid
HNO3 (aq) = nitric acid
(polyatomic ion) -ide +ic acid
HCN (aq) = cyanic acid
(polyatomic ion) -ite +ous acid
HNO2 (aq) = nitrous acid

11. Formula Writing of Acids
Acids formulas get written like any other. Write the H+1 first, then figure out what the negative ion is based on the name. Cancel out the charges to write the formula. Don’t forget the (aq) after it…it’s only an acid if it’s in water!
Hydrosulfuric acid: H+1 and S-2 = H2S (aq)
Carbonic acid: H+1 and CO3-2 = H2CO3 (aq)
Chlorous acid: H+1 and ClO2-1 = HClO2 (aq)
Hydrobromic acid: H+1 and Br-1 = HBr (aq)
Hydronitric acid:
Hypochlorous acid:
Perchloric acid:

12. Formulas, Naming and Properties of Bases
Arrhenius Definition of Bases: ionic compounds that dissolve in water to produce OH- (hydroxide) as the only negatively charged ion in solution.
NaOH (s)  Na+1 (aq) + OH-1 (aq)
Properties of Bases
Naming of Bases
Formula Writing of Bases

13. Properties of Bases
Bases react with fats to form soap and glycerol. This process is called saponification.
Bases have a pH of more than 7.
Dilute solutions of bases taste bitter.
Bases turn phenolphthalein PINK, litmus BLUE and bromthymol blue BLUE.
Bases neutralize acids.
Bases are formed when alkali metals or alkaline earth metals react with water. The words “alkali” and “alkaline” mean “basic”, as opposed to “acidic”.

14. Naming of Bases
Bases are named like any ionic compound, the name of the metal ion first (with a Roman numeral if necessary) followed by “hydroxide”.
Fe(OH)2 (aq) = iron (II) hydroxide
Fe(OH)3 (aq) = iron (III) hydroxide
Al(OH)3 (aq) = aluminum hydroxide
NH3 (aq) is the same thing as NH4OH:
NH3 + H2O  NH4OH
Also called ammonium hydroxide.

15. Formula Writing of Bases
Formula writing of bases is the same as for any ionic formula writing. The charges of the ions have to cancel out.
Calcium hydroxide = Ca+2 and OH-1 = Ca(OH)2 (aq)
Potassium hydroxide = K+1 and OH-1 = KOH (aq)
Lead (II) hydroxide = Pb+2 and OH-1 = Pb(OH)2 (aq)
Lead (IV) hydroxide = Pb+4 and OH-1 = Pb(OH)4 (aq)
Lithium hydroxide =
Copper (II) hydroxide =
Magnesium hydroxide =