Acids and Bases Flashcards
Memorize acids and bases
hydronium ion
H₃O⁺
hydroxide ion
OH⁻
Kw expression
Kw=[H3O+][OH−]=1.0 × 10−14
At 25 °C, the value of Kw is
1.0 × 10^−14
pH+pOH=
14.00
acidic classified as (pH)
[H3O+] > [OH−]
pH < 7
neutral classified as (pH)
[H3O+] = [OH−]
pH = 7
basic classified as (pH)
[H3O+] < [OH−]
pH > 7
6 strong ACIDS
HCIO4 - perchloric acid
HCl - hydrochloric acid
HBr - hydrobromic acid
HI - hydroiodic acid
HNO3 - nitric acid
H2SO4 - sulfuric acid
6 strong BASES
LiOH - lithium hydroxide
NaOH - sodium hydroxide
KOH - potassium hydroxide
Ca(OH)2 - calcium hydroxide
Sr(OH)2 - strontium hydroxide
Ba(OH) 2 - barium hydroxide
Arrhenius Acids and Bases
acids are substances that produces H+ when dissolved in water and bases are substances that produces OH- when dissolved in water
amines are _ _
weak bases
Bronsted-Lowry Acids and Bases
acids are a proton (H+) donor and bases are a proton (H+) acceptor
the stronger the acid…
the weaker it’s conjugate base will be
the stronger the base…
the weaker its conjugate acid will be
NH3 is an important _ _
weak base
the larger the Ka, the _ the acid
stronger
the larger the Kb, the _ the base
stronger
strong bases and acids have _ ionization
100%
What is the molarity of water?
55.5 M
monoprotic acid has _ proton(s) it can donate
one
diprotic acid has _ proton(s) it can donate
two
triprotic acid has _ proton(s) it can donate
three
polyprotic acids
diprotic and triprotic acids
For weak polyprotic acids, Ka1 _ Ka2
Ka1 > Ka2
Ka1 will be greater than Ka2 ALWAYS
EXCEPT for _, treat all polyprotic acids as monoprotic acids
H2SO4 (sulfuric acid)
In polyprotic acids, assume all of _ comes from the first step
H3O+
a salt is composed of a _ and an _
cation, anion
If the cation is a Group _ or _ cation and the anion is from a STRONG acid, the salt will be _
IA, IIA, neutral
spectator ions
do not react with water, they “spectate”
strong _ cannot be formed in water
ACIDS
common ion effect
ionization of a weak acid is suppressed by the presence of an ion in common with the acid
buffer solutions resist change in _ when small amounts of a strong acid/base are added
pH
buffer solution consists of _ _ and its conjugate _ present in significant amounts
weak acid, base
what equation holds true to every aqueous solution
H2O (l) + H2O (l) <=> H3O+ (aq) + OH- (aq)
optimal buffer =
1
an optimal buffer can _ just as much added acid as added base
neutralize
for a solution to be a buffer, it should be between
0.1-10
buffer capacity
amount of acid or base that can be added to a given volume of a buffer solution before its pH changes significantly
the higher the concentrations of _ components…
the more capacity they hold
