1. Hydrolysis and Neutralization
Acids and Bases:
salt hydrolysis
pH pH 8.9
pH 5.3
Hydrolysis and Neutralization

2. C12-5-11 NEUTRALIZATION AND SOLUTION
OUTCOME QUESTION(S):
C NEUTRALIZATION AND SOLUTION
Write balanced neutralization reactions involving strong acids and bases.
Using a standardized acid or base, determine the concentration of an unknown base or acid.
Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula.
Vocabulary & Concepts
salt hydrolysis

3. Neutralization reaction
Acid + Base H2O + salt
Salt: ionic compound produced by reacting acid with base
HCl(aq) + NaOH(aq)
H2O(l) +
Na+
Cl-
(aq)
Hydrolysis: breakdown by water
Salt Hydrolysis:
The produced salt dissociates in solution and may react with water to produce an acidic/basic solution.
When a reactant in the neutralization is weak it will generally result in a solution that is NOT neutral. 

4. Na+ Cl- HCl(aq) + NaOH(aq) H2O(l) +
3 possible neutralization outcomes:
Strong Acid + Strong Base
HCl(aq) + NaOH(aq)
H2O(l) +
Na+
Cl-
(aq)
Acid to Base
Base to Acid
Water is neutral
Na+ is unreactive
Cl- is unreactive
Equivalence results in neutral solution pH = 7
No product has characteristics of an acid/base
Strong acid/base leave behind weak conjugates

5. NH4+ is a strong conjugate acid created from weak base NH3
Strong Acid + Weak Base
NH3(aq) + HNO3(aq)
H2O(l) +
NH4+
NO3-
(aq)
NH4+ is a strong conjugate acid created from weak base NH3
NH4+(aq) + H2O (aq) H3O+(aq) + NH3 (aq)
Acid to Base
Base to Acid
Note: sloppy
s-curves
Equivalence results in acidic solution pH < 7
A strong conjugate acid has been produced

6. CH3COO- is a strong conjugate base created from weak acid CH3COOH
Weak Acid + Strong Base
CH3COOH(aq) + NaOH(aq)
H2O(l) +
Na+
CH3COO-
(aq)
CH3COO- is a strong conjugate base created from weak acid CH3COOH
CH3COO-(aq) + H2O (aq) OH-(aq) + CH3COOH (aq)
Acid to Base
Base to Acid
Note: sloppy
s-curves
Equivalence results in basic solution pH > 7
A strong conjugate base has been produced

7. Anions of strongest acids are unreactive:
What to look for:
Anions of strongest acids are unreactive:
Cl-, ClO4-, I-, Br-, NO3- (weakest CBs)
Metal cations of strongest bases are unreactive:
Alkali (I) and Earth (II) metals (weakest CAs)
SALT
Cation
Anion
Is it a group I or II metal?
Is it part of a strong acid?
YES NO NO
YES
No effect
(neutral)
No effect
(neutral)
Could hydrolyze
WILL hydrolyze

8. It says “could” because not all metal cations will affect pH
SALT
Cation
Anion
Is it a group I or II metal?
Is it part of a strong acid?
YES NO NO
YES
NO effect
(neutral)
Na+ K+
Mg2+
(etc.)
Could hydrolyze
NH4+
Fe3+
Sn2+
(etc.)
NO effect
(neutral)
ClO4- I-
NO3-
(etc.)
WILL hydrolyze
O2- F-
NO2-
(etc.)
It says “could” because not all metal cations will affect pH
Notice: Cations generally create acidic solutions, while anions generally create basic solutions

9. Both solutions are basic
Are K2CO3 and MgS acidic, basic or neutral?
Step 1. Identify the ions present:
How will they dissociate in water?
Look for the anions on the Strength Chart…
No effect
(Group I)
No effect
(Group II)
K2CO3(s)
→ 2 K+(aq) + CO32–(aq)
MgS(s)
→ Mg2+(aq) + S2–(aq)
Strong conjugate base of weak acid HCO3-
Strong conjugate base of weak acid HS-
Step 2. Determine if each ion will affect the pH:
What acid or base reaction did it come from?
CO32-(aq) + H2O (aq) OH-(aq) + HCO3- (aq)
Both solutions
are basic
S2-(aq) + H2O (aq) OH-(aq) + HS- (aq)

10. C12-5-11 NEUTRALIZATION AND SOLUTION
CAN YOU / HAVE YOU?
C NEUTRALIZATION AND SOLUTION
Write balanced neutralization reactions involving strong acids and bases.
Using a standardized acid or base, determine the concentration of an unknown base or acid.
Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula.
Vocabulary & Concepts
salt hydrolysis