1. Hydrolysis and Neutralization

2. Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula.

3. Ionic compound produced by reacting an acid with a base.
Neutralization reaction:
acid + base salt + water
Ionic compound produced by reacting an acid with a base.
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
Salt produced in a neutralization can react with the water to produce acidic or basic solutions.
We call this process salt hydrolysis.

4. NH4+(aq) + H2O (aq) H3O+(aq) + NH3 (aq)
Salt anions may accept hydrogen ions from the water producing a basic solution. OR
Salt cations may donate hydrogen ions to the water producing an acidic solution.
HNO3(aq) + NH3 (aq) NH4NO3 (aq) + H2O(l)
NH4+(aq) + NO3¯(aq)
NH4+(aq) + H2O (aq) H3O+(aq) + NH3 (aq)

5. Basic salts result from the reaction of a strong base with a weak acid.
CH3COOH(aq) + NaOH (aq) CH3COONa (aq) + H2O(l)
Na+(aq) + CH3COO¯(aq)
CH3COO-(aq) + H2O(l) OH-(aq) + CH3COOH (aq)

6. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
3 possible neutralization reactions:
SA + SB - results in neutral solution, pH = 7
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
Anions of strong acids won’t affect pH:
Cl-, ClO4-, I-, Br-, NO3-
WA + SB - produces a solution with pH > 7
SA + WB – produces a solution with pH < 7

7. Is K2CO3, acidic, basic or neutral?
Step 1. Identify the ions present.
Potassium carbonate will dissociate in water
K2CO3(s) → 2 K+(aq) + CO32–(aq)
Step 2. Determine if each ion will affect the pH.
Carbonate ion is a strong CB of weak acid HCO3– .
CO32– (aq) + H2O (l)  HCO3– (aq) + OH– (aq)
Solution is basic.

8. FeCl3 is acidic in water:
Other Salts:
Metal salts containing 3+ or 2+ transition metal ions, will be acidic in water.
FeCl3 is acidic in water:
Fe(H2O) H2O  H3O Fe(H2O)5(OH)2+
Oxides are basic in water because oxide ion, O2–, is a strong base. – (Na2O)
O2–(aq) + H2O(l) → OH–(aq) + OH–(aq)