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Drill: Calculate the pH of 0.10 M H 2 Z in 0.50 M KHZ. K a1 = 2.0 x 10 -5 K a2 = 5.0 x 10 -9

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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

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

Salts

- Ionic compounds that dissolve ~ 100 % in water

- When salts dissolve, their ions can recombine with water

Salt Solutions

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

- The salts of weak bases can recombine with water producing acidic 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.KaHBz = 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

- 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
- Kb = 2.5 x 10-5

AP CHM HW

- Read: Chapter 14
- Problems: 43
- Page: 422

- Read: Chapter 18
- Problems: 83
- Page: 790

- Salts of strong acids & weak bases make acidic solutions

- Salts of strong bases & weak acids make basic solutions

- Salts of strong acids & strong bases make neutral solutions

- NaAc MnCl2
- KNO3 NH4Br
- KHSO4 NH4Ac

- KAc NaCl
- KClO2 NH4Cl
- K2SO4 NaI

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

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

- Metal oxides that form bases when added to water

- Na2O SO2
- NO2 CO2
- CaO Al2O3

Calculate the pH of a solution of 0.30 M KQ.

- KaHQ = 3.0 x 10-5

AP CHM HW

- Read: Chapter 14
- Problems: 35
- Page: 422

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

AP Test

- Thursday

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

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

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 10-2Ka2 = 6.0 x 10-8

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

Strong Bases

Base rxns

KW, KA, KB, & pH

Calculate pH of:

- 0.025 M HNO3
- 0.020 M KOH

- 0.20 M HNO2
- Ka = 2.0 x 10-4

- 3.0 M HZin
- 2.0 M KZ
- Ka HZ = 3.0 x 10-5

- 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. 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 10-3Ka2 = 5.0 x 10-8Ka3 = 2.5 x 10-13

- 2.0 M HQ
- Ka = 2.0 x 10-6

- 0.60 M HZin
- 0.90 M KZ
- Ka HZ = 3.0 x 10-5

- 0.20 M KQ
- Ka HQ = 2.0 x 10-7

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