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

Hydrolysis

Water is added to decompose something

Hydrolysis

MX + HOH

HX + MOH

- Ionic compounds that dissolve ~ 100 % in water

Salts of Acids

- Salts of acids are negative
(A-)

Salts of Bases

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

Salt Solutions

- When salts dissolve, their ions can recombine with water

- 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 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 Problem

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

Salt Problem

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

Drill:

Calculate the pH of a 0.18 M solution of KC2H3O2

- Ka = 1.8 x 10-5

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

CHM II HW

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

Drill:

Calculate the pH of a 0.16 M solution of KC7H5O2

- Ka = 6.4 x 10-5

Salt Applications

- Salts of strong acids & weak bases make acidic solutions

Salt Applications

- Salts of strong bases & weak acids make basic solutions

Salt Applications

- Salts of strong acids & strong bases make neutral solutions

Predict Relative pH

- NaAcMnCl2
- KNO3NH4Br
- KHSO4NH4Ac

Predict Relative pH

- KAcNaCl
- KClO2NH4Cl
- K2SO4NaI

Anhydrides

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

Acid Anhydrides

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

Basic Anhydrides

- Metal oxides that form bases when added to water

Predict Relative pH

- Na2OSO2
- NO2CO2
- CaOAl2O3

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

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

CHM II HW

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

- 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 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 1.0 M KH2PO4 in 0.50 M K2HPO4. Ka1 = 7.5 x 10-3Ka2 = 6.2 x 10-8Ka3 = 4.2 x 10-13

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

Calculate pH of:

0.20 M MOHin

0.50 M MCl

Kb = 5.0 x 10-5

Calculate pH of:

0.20 M MCl

Kb = 5.0 x 10-5

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

Arhenius, Bronsted-Lowry, & Lewis Acids & Bases

Strong Acids

Strong Bases

Acid rxns

Base rxns

A/B Equilibrium Constants

KW, KA, KB, & pH

- 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 HZin
- 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. 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

Calculate pH of:

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

Calculate pH of:

- 0.60 M HZin
- 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