Untitled - Kelly Walsh High School

232 CHEMISTRY FOR THE UTTERLY CONFUSED
Brønsted-Lowery acids are H + donors and bases are H + acceptors. Strong acids
dissociate completely in water. Weak acids only partially dissociate, establishing
an equilibrium system. Weak acid and base dissociation constants (K a and K b)
describe these equilibrium systems. Water is amphoteric, acting as both an acid
or a base. We describe water’s equilibrium by the K w expression. A pH value is
a way of representing a solution’s acidity. Some salts and oxides have acid-base
properties. A Lewis acid is an electron pair acceptor while a Lewis base is an
electron pair donor.
1. List the strong acids.
2. List the strong bases.
3. Give the formula for the conjugate base of each of the following
a. HNO 3 b. HC 2H 3O 2 c. NH 4 d. H2SO 4 e. HCO 3
4. Give the formula for the conjugate acid of each of the following
a. Cl b. PO 4 3 c. NH3 d. NO 2 e. O 2
5. What is the relationship between the K a and the K b for any conjugate acidbase
pair?
6. What mathematical relationship defines the pH of a solution?
7. Determine the pH in each of the following
a. [H ] 10 3 M b. [H ] 1.5 10 5 M c. [H ] 1.0 M
d. [H ] 1.0 10 15 M e. pOH 4.2
8. What is the relationship between the pH and the pOH for any aqueous
solution?
9. Determine the hydrogen ion concentration in each of the following
a. pH 4 b. pH 3.75 c. pOH 7.0
d. [OH ] 3.2 10 3 M e. pH 0.50
10. Determine the pH of each of the following
a. 1.0 10 2 M HCl b. 4.5 10 5 M HNO 3 c. 1.5 10 3 M NaOH
11. Determine the [H + ] of each of the following
a. 1.0 10 1 M HC 2H 3O 2, K a 1.8 10 5
b. 4.5 10 2 M HClO 2, K a 1.1 10 2
c. 1.5 M HCO 3 , Ka 4.8 10 11
12. Determine the pH of each of the solutions in question 11.
13. Determine the [OH ], pOH, and pH of a 0.100 M solution of ammonia,
NH 3. K b 1.8 10 5
ANSWER KEY
1. Chloric acid, HClO 3, Hydrobromic acid, HBr, Hydrochloric acid, HCl,
Hydroiodic acid, HI, Nitric acid, HNO 3, Perchloric acid, HClO 4, Sulfuric
acid, H 2SO 4