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

Salt orHydrolysis Reactions

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

HydrolysisWater is added to decompose something

HydrolysisMX + HOH

HX + MOH

Salts

SaltsIonic compounds that dissolve ~ 100 % in water

Salts of AcidsSalts of acids are negative(A-)

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

Salt SolutionsWhen salts dissolve, their ions can recombine with water

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

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

Salt SolutionsA- + 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

Salt or Hydrolysis Problems

Salt ProblemCalculate the pH of a 0.20 M solution of NaBzKa HBz = 6.4 x 10-5

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

Salt ProblemCalculate the pH of a 0.20 M solution of KNO2Ka HNO2 = 7.1 x 10-4

Salt ProblemCalculate the pH of a 0.10 M solution of R-NH3ClKb R-NH2 = 2.5 x 10-5

Calculate the pH of a 0.18 M solution of KC2H3O2Ka = 1.8 x 10-5

Drill: Calculate the salt to acid ratio required to make a buffer solution with a pH of 4.495 using benzoic acid.Ka HBz = 6.4 x 10-5

Salt ApplicationsSalts of strong acids & weak bases make acidic solutions

Salt ApplicationsSalts of strong bases & weak acids make basic solutions

Salt ApplicationsSalts of strong acids & strong bases make neutral solutions

Predict Relative pHNaAcMnCl2KNO3NH4BrKHSO4NH4Ac

Predict Relative pHKAcNaClKClO2NH4ClK2SO4NaI

AnhydridesCompounds without water; that when added to water, form other compounds

Acid AnhydridesNon-metal oxides that form acids when added to water

Basic AnhydridesMetal oxides that form bases when added to water

Predict Relative pHNa2OSO2NO2CO2CaOAl2O3

Calculate the pH of a 0.16 M solution of KC7H5O2Ka = 6.4 x 10-5

Calculate the pH of a solution of 0.0030 M KQ.Ka HQ = 3.0 x 10-5

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

Are there any questions on previous material?

A/B eq, Buffer & Salt Hydrolysis Problem

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

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.

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 10-7Ka2 = 4.8 x 10-11

Drill: Calculate the pH of0.10 M HF. Ka HF = 6.5 x 10-4

Test Review

Expect a straight acid/base problem like the drill

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

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

Predict Relative pHK2OMgOClO2(NH4)2OSO3N2O3

Predict Relative pHKAcNaClKClO2NH4ClK2SO4NaI

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 MClKb = 5.0 x 10-5

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

Drill: Calculate the pH of0.20 M KQ. Ka HQ = 8.0 x 10-5

Calculate pH of:0.20 M HNO2Ka = 2.0 x 10-4

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

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

Calculate pH of:2.0 M HQKa = 2.0 x 10-6

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

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

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 HNO30.020 M KOH

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 10-7Ka2 = 4.7 x 10-11

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

The take-home portion of the test is due by 8:15 tomorrow