Chemistry 12 Unit 5
ACIDS AND BASES SUMMARY NOTES
ARRENHIUS THEORY
ACID – releases H+
v4.2
BASE – releases OH-
BRONSTED-LOWRY THEORY ACID – proton donor
BASE – proton acceptor
Conjugate pairs differ by one proton (H+)
Amphiprotic – can act as an acid or a base (usually negative and
have an easily removable hydrogen.)
NEUTRALIZATION – Acid + Base  Salt + Water
ACIDS
-taste sour
-conduct electricity
-turn litmus RED
-produce H2(g) when reacting with
certain metals (ex. Mg)
-neutralized by bases
BASES
-taste bitter
-conduct electricity
-turn litmus BLUE
-feel slippery
-neutralized by acids
Both acids and bases conduct electricity, the amount that it conducts depends on the
number of ions in solution. More ions = more conductive. (Strong acid/base will have a
higher conductivity that weak acids and bases of the same concentration)
STRONG ACIDS/BASES – Ionize 100% (not at equilibrium)
WEAK ACIDS/BASES – less than 100% ionized (at equilibrium – use ICE chart to solve)
Ka/b = [products]
[reactants]
STRONGER ACIDS AND BASES WILL REACT TO PRODUCE
THEIR WEAKER CONJUGATES
SELF-IONIZATION OF WATER
2H2O(l) + 59kJ  H3O+(aq) + OH-(aq)
Kw = [H3O+][OH-]
pKw = pH + pOH
Kw = 1.00 x 10-14 @ 25oC
pH = -log[H3O+]
pOH = -log[OH-]
[H3O+] = antilog(-pH)
[OH-] = antilog(-pOH)
pH + pOH = pKw (which is 14.00 @ 25oC)
(If temp changes, Kw changes)
@25oC
pH < 7 = ACIDIC
pH = 7 = NEUTRAL
pH > 7 = BASIC