Unit 13 Quiz Topics
Multiple Choice
Know Arrhenius Definition of Acids
Know Bronsted Lowry Definition of Acids
Acids, Base, Conjugate Acid, Conjugate Base
pH scale, which ones are acids and which ones are bases?
How do you calculate pH and pOH
Strong Acids Definition
Properties of acids and bases
Free Response
Naming Acids (HW #2)
Writing the correct Formula (HW #1)
Neutralization Reactions-Arrhenius Acid/Base Reactions
(HW#3)
Bronsted-Lowry Acid Base Equations (HW #4)
Properties of Acids and Bases
-Acids
 tastes sour
 conduct electricity
 reacts with metals to form gas
 changes indicators (litmus red)
 reacts with hydroxides to form
water and a salt
-Base
 tastes bitter
 feels slippery
 changes indicators (litmus blue)
 reacts with acids to form water
and a salt
pH scale
 pH = - log[H+]
 pOH = -log[OH-]
 acidic solutions, pH < 7
 basic solutions, pH > 7
 neutral solutions, pH = 7
 pH + pOH = 14
Arrhenius Acid/Base
 Acids produce hydrogen ions (H+)
 Bases produce hydroxide ions
(OH-)
Neutralization Reactions
 Acid + Base  Salt + Water
Naming Acids
 -ide, use hydro prefix, -ic ending
 -ate, no hydro prefix, -ic ending
 -ite, no hydro prefix, -ous ending
Bronsted Lowry Acid/Base
An acid is a proton (H+) donor and
a base is a proton acceptor.
 Conjugate Acid – an acid on the
reactant side produces a conjugate
base on the product side
 Conjugate Base – the base on the
reactant side produces a conjugate
acid.
Strengths of Acid/Bases
 Strong Acids and bases completely
ionize.
 Weak acids and bases do not
completely ionize.
Polyatomic Ions
Acetate
CH3CO2Ammonium NH4+
Carbonate
CO32Chlorate
ClO3Chlorite
ClO2Chromate
CrO42Cyanide
CNHydroxide
OHNitrate
NO3Nitrite
NO2Perchlorate ClO4Phosphate PO43Phosphite
PO33Sulfate
SO42Sulfite
SO32