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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 - PowerPoint PPT Presentation

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

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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

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

MX + HOH

HX + MOH

• Ionic compounds that dissolve ~ 100 % in water

• Salts of acids are negative

(A-)

• Salts of bases are Positive

(M+ or B+)

• When salts dissolve, their ions can recombine with water

• 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: benzoic acid & sodium benzoate at a pH of 5.00.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 benzoic acid & sodium benzoate at a pH of 5.00.

Salt Problem benzoic acid & sodium benzoate at a pH of 5.00.

• Calculate the pH of a 0.20 M solution of NaBz

• Ka = 6.4 x 10-5

Salt Problem benzoic acid & sodium benzoate at a pH of 5.00.

• Calculate the pH of a 0.10 M solution of R-NH3Cl

• Kb = 2.5 x 10-5

Drill: benzoic acid & sodium benzoate at a pH of 5.00.

Calculate the pH of a 0.18 M solution of KC2H3O2

• Ka = 1.8 x 10-5

AP CHM HW benzoic acid & sodium benzoate at a pH of 5.00.

• Problems: 43

• Page: 422

CHM II HW benzoic acid & sodium benzoate at a pH of 5.00.

• Problems: 83

• Page: 790

Drill: benzoic acid & sodium benzoate at a pH of 5.00.

Calculate the pH of a 0.16 M solution of KC7H5O2

• Ka = 6.4 x 10-5

Short Test Friday benzoic acid & sodium benzoate at a pH of 5.00.

Salt Applications benzoic acid & sodium benzoate at a pH of 5.00.

• Salts of strong acids & weak bases make acidic solutions

Salt Applications benzoic acid & sodium benzoate at a pH of 5.00.

• Salts of strong bases & weak acids make basic solutions

Salt Applications benzoic acid & sodium benzoate at a pH of 5.00.

• Salts of strong acids & strong bases make neutral solutions

Predict Relative pH benzoic acid & sodium benzoate at a pH of 5.00.

• NaAc MnCl2

• KNO3 NH4Br

• KHSO4 NH4Ac

Predict Relative pH benzoic acid & sodium benzoate at a pH of 5.00.

• KAc NaCl

• KClO2 NH4Cl

• K2SO4 NaI

Anhydrides benzoic acid & sodium benzoate at a pH of 5.00.

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

Acid Anhydrides benzoic acid & sodium benzoate at a pH of 5.00.

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

Basic Anhydrides benzoic acid & sodium benzoate at a pH of 5.00.

• Metal oxides that form bases when added to water

Predict Relative pH benzoic acid & sodium benzoate at a pH of 5.00.

• Na2O SO2

• NO2 CO2

• CaO Al2O3

AP CHM HW benzoic acid & sodium benzoate at a pH of 5.00.

• Problems: 35

• Page: 422

CHM II HW benzoic acid & sodium benzoate at a pH of 5.00.

• Problems: 67 & 75

• Page: 789-790

Drill: Calculate the pH of a 0.72 M NH benzoic acid & sodium benzoate at a pH of 5.00.4NO3 solution.KbNH3 = 1.8 x 10-5

A/B eq, Buffer & Salt Hydrolysis Problems benzoic acid & sodium benzoate at a pH of 5.00.

AP Test benzoic acid & sodium benzoate at a pH of 5.00.

• Thursday

11.2 g of KOH was added to 2.0 L of 0.075 M H benzoic acid & sodium benzoate at a pH of 5.00.2CO3. 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. buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.Ka HF = 6.5 x 10-4

Calculate [H buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.3PO4], [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 0.10 M HF in 0.20 M NaF. buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.Ka HF = 6.5 x 10-4

Calculate the pH of 5.0 M KCN. buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.KaHCN= 5.0 x 10-10

Calculate pH of: buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.

0.20 M MOHin

0.50 M MCl

Kb = 5.0 x 10-5

Calculate pH of: buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.

0.20 M MCl

Kb = 5.0 x 10-5

Drill: Calculate the pH of buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.0.20 M KQ. KaHQ = 8.0 x 10-5

1.5 L of 0.25 M Ba(OH) buffering capacity at pH ~ 5.4. In general terms, describe what acid or base you would chose, & how you would make the buffer.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

Strong Acids Salt Equilibria

Strong Bases

Acid rxns Salt Equilibria

Base rxns

A/B Equilibrium Constants Salt Equilibria

KW, KA, KB, & pH

Calculate pH of: Salt Equilibria

• 0.025 M HNO3

• 0.020 M KOH

Calculate pH of: Salt Equilibria

• 0.20 M HNO2

• Ka = 2.0 x 10-4

Calculate pH of: Salt Equilibria

• 3.0 M HZin

• 2.0 M KZ

• Ka HZ = 3.0 x 10-5

Calculate pH of: Salt Equilibria

• 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 H Salt Equilibria2CO3. Calculate [H2CO3], [HCO3-], [CO3-2], [H+], [OH-], & pH of the solution.Ka1 = 4.4 x 10-7Ka2 = 4.7 x 10-11

Calculate [H Salt Equilibria3A], [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: Salt Equilibria

• 2.0 M HQ

• Ka = 2.0 x 10-6

Calculate pH of: Salt Equilibria

• 0.60 M HZin

• 0.90 M KZ

• Ka HZ = 3.0 x 10-5

Calculate pH of: Salt Equilibria

• 0.20 M KQ

• Ka HQ = 2.0 x 10-7