Drill: Calculate the pH of 0. 10 M H2Z in 0. 50 M KHZ. Ka1 = 2 Drill: Calculate the pH of 0.10 M H2Z in 0.50 M KHZ. Ka1 = 2.0 x 10-5 Ka2 = 5.0 x 10-9

Hydrolysis Reactions

Hydrolysis Any reaction in which water is decomposed with all or part of its decomposition portions combining with the products

Water is added to decompose something Hydrolysis Water is added to decompose something

Hydrolysis MX + HOH HX + MOH

Salts

Ionic compounds that dissolve ~ 100 % in water Salts Ionic compounds that dissolve ~ 100 % in water

Salts of acids are negative

Salts of bases are Positive (M+ or B+)

When salts dissolve, their ions can recombine with water Salt Solutions When salts dissolve, their ions can recombine with water

Salt Solutions The salts of weak acids can recombine with water producing basic solutions

Salt Solutions The salts of weak bases can recombine with water producing acidic solutions

Salt Solutions A- + H2O HA + OH- B+ + H2O H+ + BOH

Drill: Calculate the salt/acid ratio of a solution of benzoic acid & sodium benzoate at a pH of 5.00. Ka HBz = 6.4 x 10-5

Drill: Calculate the pH of a solution of 0. 10 M NH3 in 0. 20 NH4Cl Drill: Calculate the pH of a solution of 0.10 M NH3 in 0.20 NH4Cl. Kb NH3 = 1.8 x 10-5

Salt or Hydrolysis Problems

Calculate the pH of a 0.20 M solution of NaBz Salt Problem Calculate the pH of a 0.20 M solution of NaBz Ka = 6.4 x 10-5

Calculate the pH of a 0.10 M solution of R-NH3Cl Salt Problem Calculate the pH of a 0.10 M solution of R-NH3Cl Kb = 2.5 x 10-5

Calculate the pH of a 0.18 M solution of KC2H3O2 Drill: Calculate the pH of a 0.18 M solution of KC2H3O2 Ka = 1.8 x 10-5

AP CHM HW Read: Chapter 14 Problems: 43 Page: 422

CHM II HW Read: Chapter 18 Problems: 83 Page: 790

Calculate the pH of a 0.16 M solution of KC7H5O2 Drill: Calculate the pH of a 0.16 M solution of KC7H5O2 Ka = 6.4 x 10-5

Short Test Friday

Salts of strong acids & weak bases make acidic solutions Salt Applications Salts of strong acids & weak bases make acidic solutions

Salts of strong bases & weak acids make basic solutions Salt Applications Salts of strong bases & weak acids make basic solutions

Salts of strong acids & strong bases make neutral solutions Salt Applications Salts of strong acids & strong bases make neutral solutions

Predict Relative pH NaAc MnCl2 KNO3 NH4Br KHSO4 NH4Ac

Predict Relative pH KAc NaCl KClO2 NH4Cl K2SO4 NaI

Anhydrides Compounds without water; that when added to water, form other compounds

Non-metal oxides that form acids when added to water Acid Anhydrides Non-metal oxides that form acids when added to water

Metal oxides that form bases when added to water Basic Anhydrides Metal oxides that form bases when added to water

Predict Relative pH Na2O SO2 NO2 CO2 CaO Al2O3

Calculate the pH of a solution of 0.30 M KQ. Ka HQ = 3.0 x 10-5

AP CHM HW Read: Chapter 14 Problems: 35 Page: 422

CHM II HW Read: Chapter 18 Problems: 67 & 75 Page: 789-790

Drill: Calculate the pH of a 0. 72 M NH4NO3 solution. Kb NH3 = 1 Drill: Calculate the pH of a 0.72 M NH4NO3 solution. Kb NH3 = 1.8 x 10-5

A/B eq, Buffer & Salt Hydrolysis Problems

AP Test Thursday

11. 2 g of KOH was added to 2. 0 L of 0. 075 M H2CO3 11.2 g of KOH was added to 2.0 L of 0.075 M H2CO3. Calculate the molarity of all ions present in the solution. Ka1 = 4.4 x 10-7 Ka2 = 4.8 x 10-11

You need to make a buffer solution with its greatest buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.

Calculate the pH of 0.10 M HF. Ka HF = 6.5 x 10-4

Calculate [H3PO4], [H2PO4-1], [HPO4-2], [PO4-3], [K+], [H+], & pH of 1 Calculate [H3PO4], [H2PO4-1], [HPO4-2], [PO4-3], [K+], [H+], & pH of 1.0 M KH2PO4 in 0.50 M K2HPO4. Ka1 = 7.5 x 10-3 Ka2 = 6.2 x 10-8 Ka3 = 4.2 x 10-13

Calculate the pH of 0.10 M HF in 0.20 M NaF. Ka HF = 6.5 x 10-4

Calculate the pH of 5.0 M KCN. KaHCN= 5.0 x 10-10

Calculate pH of: 0.20 M MOH in 0.50 M MCl Kb = 5.0 x 10-5

Calculate pH of: 0.20 M MCl Kb = 5.0 x 10-5

Drill: Calculate the pH of 0.20 M KQ. Ka HQ = 8.0 x 10-5

1. 5 L of 0. 25 M Ba(OH)2 was added to 1. 0 L of 0. 60 M H2SO3 1.5 L of 0.25 M Ba(OH)2 was added to 1.0 L of 0.60 M H2SO3. Calculate [H2SO3], [HSO3-], [SO3-2], [H+], [OH-], & pH of the solution. Ka1 = 1.7 x 10-2 Ka2 = 6.0 x 10-8

Review of Acid/Base descriptions and Acid/Base, Buffer, & Salt Equilibria

Arhenius, Bronsted-Lowry, & Lewis Acids & Bases

Strong Acids Strong Bases

Acid rxns Base rxns

A/B Equilibrium Constants KW, KA, KB, & pH

Calculate pH of: 0.025 M HNO3 0.020 M KOH

Calculate pH of: 0.20 M HNO2 Ka = 2.0 x 10-4

Calculate pH of: 3.0 M HZ in 2.0 M KZ Ka HZ = 3.0 x 10-5

Calculate pH of: 0.20 M KR Ka HR = 2.0 x 10-5

150 mL of 0. 10 M KOH was added to 100. 0 mL of 0. 10 M H2CO3 150 mL of 0.10 M KOH was added to 100.0 mL of 0.10 M H2CO3. Calculate [H2CO3], [HCO3-], [CO3-2], [H+], [OH-], & pH of the solution. Ka1 = 4.4 x 10-7 Ka2 = 4.7 x 10-11

Calculate [H3A], [H2A-1], [HA-2], [A-3], [K+], [H+], [OH-], & pH of 2 Calculate [H3A], [H2A-1], [HA-2], [A-3], [K+], [H+], [OH-], & pH of 2.0 M KH2A. Ka1 = 4.0 x 10-3 Ka2 = 5.0 x 10-8 Ka3 = 2.5 x 10-13

Calculate pH of: 2.0 M HQ Ka = 2.0 x 10-6

Calculate pH of: 0.60 M HZ in 0.90 M KZ Ka HZ = 3.0 x 10-5

Calculate pH of: 0.20 M KQ Ka HQ = 2.0 x 10-7