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 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


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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. 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 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 Reactions


Hydrolysis

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


Salts


Salts

  • 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


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.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


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


AP CHM HW

  • 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


Short Test Friday


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


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.KbNH3 = 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. 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 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 MOHin

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 of0.20 M KQ. KaHQ = 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. 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


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 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


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