The document provides information about acid-base chemistry including: 1) Calculating the concentration of H+ ions and determining if solutions are acidic or basic based on the relative concentrations of H+ and OH- ions. 2) Defining pH as the negative logarithm of the H+ ion concentration and calculating pH values from given [H+] values. 3) Relating pH and pOH through the equation pH + pOH = 14. 4) Listing the 7 strong acids and their formulas as well as the 7 strong bases and their formulas.

1. KEY
GENERAL CHEMISTRY-II (1412)
S.I. # 20
1. Calculate the concentration of H+ (aq) in (a) a solution in which [OH-] is 0.010 M,
(b) a solution in which [OH-] is 1.8x10-9 M.
a. using [H+][OH-] = 1.0 x 10-14
[H+] = 1.0 x 10-14 = 1.0 x 10-14 = 1.0 x 10-12M
[OH-] 0.010
The solution is basic because [OH-] > [H+]
b. [H+] = 1.0 x 10-14 = 1.0 x 10-14 = 3.6 x 10-6M
[OH-] 1.8 x 10-9
The solution is acidic because [H+] > [OH-]
2. Define pH and give the formula by which it is calculated.
The molar concentration of H+ (aq) in an aqueous solution is usually very small.
For convenience, we therefore usually express [H+] in terms of pH, which is the negative
logarithm in base 10 of [H+].
pH = -log[H+]
3. Calculate the pH of a solution when the value of [H+] is 1.0 x 10-7M and when [H+]
is 1.0 x 10-3M.
pH = -log (1.0 x 10-7) = -(-7.00) = 7.00 = Neutral
pH = -log (1.0 x 10-3) = -(-3.00) = 3.00 = Acidic
4. Give the pH of a solution when the value of [OH-] is 2.0 x 10-3M.
[H+] = Kw = 1.0 x 10-14 = 5.0 x 10-12M
[OH-] 2.0 x 10-3
pH = -log (5.0 x 10-12) = 11.30 = Basic
5. Determine [H+] if the pH of a sample is 3.76.
pH = -log[H+] = 3.76
log[H+] = -3.76
[H+] = antilog(-3.76) = 10-3.76 = 1.7 x 10-4M.

2. KEY
6. Provide the equation for determining pOH and show how it is related to pH.
pOH = -log[OH-]
take the negative log of both sides  -log[H+] + (-log[OH-]) = -log Kw
we obtain the following expression: pH + pOH = 14.00 at 25°C.
7. List the names and formulas for the 7 strong acids and the 7 strong bases.
7 STRONG ACIDS 7 STRONG BASES
1. HCl – hydrochloric acid NaOH – sodium hydroxide
2. HBr – hydrobromic acid KOH – potassium hydroxide
3. HI – hydroiodic acid Ba(OH)2 – barium hydroxide
4. HNO3 – nitric acid LiOH – lithium hydroxide
5. HClO3 – chloric acid RbOH – rubidium hydroxide
6. HClO4 – perchloric acid CsOH – cesium hydroxide
7. H2SO4 – hydrogen sulfate Sr(OH)2 – strontium hydroxide
8. List 3 main points of strong acids
1.Completely ionized
2. Only ions are present
3. No equilibrium
List 3 main points of weak acids
1. Not completely ionized
2. Molecules and Ions present
3. Equilibrium possible, Eq const.
9. What do weak acids and weak bases have in common?
They are weak electrolytes that ionize only to a limited extent in water and
contain Ionized and non-ionized species.
10. Why is HCl- as strong acid and a weak base?
Because Cl- will not react with H+. If it did, HCl(aq) {a strong acid} would form

3. KEY
which does not exist