CHAPTER 24 ACID, BASES, AND SALTS
24-1 Arrhenius theory
acids, bases, and salts are called electrolytes because they
conduct a current when dissolved in water
arrhenius theory: an acid produces H+ in water solution; a base
produces 0H- in water solution
24-2 Bronsted-Lowery theory
the conjugate base is the particle formed when a proton is
released by an acid
the conjugate acid of a base is formed when the base accepts a
proton form the acid
B-L theory:in a chemical reaction, any substance that donates a
proton is an acid, and any substance that accepts a proton
is a base
24-3 Lewis Theory
L theory: an acid is an electron pari acceptor; a base is an
electron pair donor
a substance that is an acid or base under the arrhenius theory
is also an acid or base under the lewis theory and bronsted- lowery theories
24-4 naming binary acids
binary acids contain only two elements
the names of binary acids begin with hydro- and end in -ic
24-5 naming ternary acids and bases
per-STEM-ic more oxygen
STEM-ic most common
STEM-ous less oxygen
hypo-STEM-ous still less oxygen
bases are named by using the name of the metallic ion and the word hydroxide
ternary acids contain 3 elements, their names depend on the
number of oxygen atoms compared to the common form
24-6 naming organic acids and bases
amines contain -NH2
carboxylic acids are named by adding the ending -oic acid to
the name of the hydrocarbon form from which the acid is
derived
24-7 acid-base behavior
metals tend to form bases; nonmetals tend to form acids
an amphoteric substance is one that can act as either an acid
or a base
for a compound HOX, if X attracts electrons strongly, the compound
will act as an acid. If X has low electronegativity, HOX
will tend to act as a base
24-8 acidic and basic anhydrides
an acidic anhydride is an oxide that produces an acid when
dissolved in water
a basic anhydride is an oxide that produces a base when dissolved
in water
anhydrous means without water
metallic oxides tend to act as basic anhydrides, forming bases
when added to water; nonmetallic oxides tend to act as acidic anhydrides
24-9 definition of a salt
an acid-base neutralization reaction produces salt + water
acidic or basic salts may be formed by neutralization reactions/
these salts are not neutral in solution
neutral-neither acidic or basic
a salt is a crystalline compound composed of the negative ion of
an acid and the positive ion of the base
24-10 strengths of acids and bases
strong acids ionize completely in water solution
strong bases dissociate completely in water solution
weak acids and bases ionize only slightly in water solution
24-11 net ionic equations
spectator ions(present in solution/not involved in the reaction)
are not involved in the reaction and are not written in the net ionic equation
some substances are written as molecules; others are written as ions
polyprotic acids have more than one ionizable hydrogen atom
rule 1: binary acids; HCl, HBr, and HI are strong-all others
are weak. strong acids are written in ionic form/weak
in molecular form
rule 2: ternary acids: if the number of oxygen atoms in the
inorganic acid molecule exceeds the number of hydrogen
atoms by 2 or more, the acid is strong. all organic
carboxylic acids are weak
rule 3: polyprotic acids:in the second and subsequent ionizations
the acids are always weak/whether or not the original acid
is strong or weak
rule 4: bases: hydroxides of the group I(IA) and 2(IIA) elements
(except beryllium) are strong bases. all others including
AMMONIA, hydroxylamine,and organic bases are weak
rule 5: salts: salts are written in ionic form if soluble,and in
undissociated form if insoluble
rule 6: oxides: oxides are always written in molecular form
rule 7: gases: are always written in molecular form
24-12 Ionization constant
Keq = [products]/[reactants]
an ionization constant Ka is a special case of an equilibrium
constant(Ka weak acid/Kb weak base)
24-13 percent of ionization
percent ionization can be calculated form the ratio obtained by
comparing the concentration of an ion in solution to the
concentration of the solute before it ionized
24-14 common ion effect
the Ka remains the same if a common ion is added
the addition of a common ion increases the concentration of one of the products of the ionization
the addition of a common ion causes the reaction to shift towards
the opposite side of the equation in accordance with
LeChatelier's principle
adding ions that are the same as those produced by the ionization
of a weak electrolyte to a solution of the electrolyte
suppresses its ionization
24-15 polyprotic acids
contains more than one ionizable hydrogen atom/ex. sulfuric acid
each successive ionization occurs to a lesser extent