3. Modified Arrhenius

4. Salt Hydrolysis/ Using Modified Arrhenius to write equations The ions of a dissolved (dissociated) salt may accept H + (aq) from water molecules OR donate H + (aq) to water molecules. This causes the solution to be slightly acidic or slightly basic depending on the direction of H + (aq) transfer. Salt Hydrolysis explains why some neutralization reactions do not result in a pH of 7.00 at the equivalence point.

5. Example # 1 NaCH 3 COO (s) dissolved in H 2 O (l) NaCH 3 COO (s) -> Na + (aq) + CH 3 COO - (aq) Ion will interact with water CH 3 COO - (aq) + H 2 O (l) ↔ Base Acid CH 3 COOH (aq) + OH - (aq) Causes the solution to be slightly basic

6. Example # 2 NH 4 Cl (s) dissolved in H 2 O (l) NH 4 Cl (s) -> NH 4 + (aq) + Cl - (aq) Ion will interact with H 2 O (l) NH 4 + (aq) + H 2 O (l) ↔ Acid Base H 3 O + (aq) + NH 3(aq)