24 Hydrolysis Chm II
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Transcript of 24 Hydrolysis Chm II
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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
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Salt orHydrolysis Reactions
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HydrolysisAny reaction in which water is decomposed with all or part of its decomposition portions combining with the products
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HydrolysisWater is added to decompose something
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HydrolysisMX + HOH
HX + MOH
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Salts
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SaltsIonic compounds that dissolve ~ 100 % in water
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Salts of AcidsSalts of acids are negative(A-)
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Salts of BasesSalts of bases are Positive(M+ or B+)
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Salt SolutionsWhen salts dissolve, their ions can recombine with water
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Salt SolutionsThe salts of weak acids can recombine with water producing basic solutions
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Salt SolutionsThe salts of weak bases can recombine with water producing acidic solutions
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Salt SolutionsA- + H2O HA + OH-
B+ + H2O H+ + BOH
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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
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Salt or Hydrolysis Problems
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Salt ProblemCalculate the pH of a 0.20 M solution of NaBzKa HBz = 6.4 x 10-5
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Drill: Calculate the pH of a solution of 0.10 M NH3 in 0.20 NH4Cl. Kb NH3 = 1.8 x 10-5
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Salt or Hydrolysis Problems
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Salt ProblemCalculate the pH of a 0.20 M solution of KNO2Ka HNO2 = 7.1 x 10-4
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Salt ProblemCalculate the pH of a 0.10 M solution of R-NH3ClKb R-NH2 = 2.5 x 10-5
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Calculate the pH of a 0.18 M solution of KC2H3O2Ka = 1.8 x 10-5
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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
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Salt ApplicationsSalts of strong acids & weak bases make acidic solutions
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Salt ApplicationsSalts of strong bases & weak acids make basic solutions
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Salt ApplicationsSalts of strong acids & strong bases make neutral solutions
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Predict Relative pHNaAcMnCl2KNO3NH4BrKHSO4NH4Ac
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Predict Relative pHKAcNaClKClO2NH4ClK2SO4NaI
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AnhydridesCompounds without water; that when added to water, form other compounds
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Acid AnhydridesNon-metal oxides that form acids when added to water
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Basic AnhydridesMetal oxides that form bases when added to water
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Predict Relative pHNa2OSO2NO2CO2CaOAl2O3
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Calculate the pH of a 0.16 M solution of KC7H5O2Ka = 6.4 x 10-5
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Calculate the pH of a solution of 0.0030 M KQ.Ka HQ = 3.0 x 10-5
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Drill: Calculate the pH of a 0.72 M NH4NO3 solution.Kb NH3 = 1.8 x 10-5
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Are there any questions on previous material?
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A/B eq, Buffer & Salt Hydrolysis Problem
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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
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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.
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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
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Drill: Calculate the pH of0.10 M HF. Ka HF = 6.5 x 10-4
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Test Review
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Expect a straight acid/base problem like the drill
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Calculate the pH of 0.10 M HF in 0.20 M KF. Ka HF = 6.5 x 10-4
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Calculate the pH of 0.10 M KF. Ka HF = 6.5 x 10-4
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Predict Relative pHK2OMgOClO2(NH4)2OSO3N2O3
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Predict Relative pHKAcNaClKClO2NH4ClK2SO4NaI
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Calculate the pH of 5.0 M KCN. KaHCN= 5.0 x 10-10
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Calculate pH of:0.20 M MOH in 0.50 M MClKb = 5.0 x 10-5
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Calculate pH of:0.20 M MClKb = 5.0 x 10-5
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Drill: Calculate the pH of0.20 M KQ. Ka HQ = 8.0 x 10-5
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Calculate pH of:0.20 M HNO2Ka = 2.0 x 10-4
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Calculate pH of:3.0 M HZ in 2.0 M KZKa HZ = 3.0 x 10-5
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Calculate pH of:0.20 M KRKa HR = 2.0 x 10-5
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Calculate pH of:2.0 M HQKa = 2.0 x 10-6
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Calculate pH of:0.60 M HZ in 0.90 M KZKa HZ = 3.0 x 10-5
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Calculate pH of:0.20 M KQKa HQ = 2.0 x 10-7
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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
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Review of Acid/Base descriptions and Acid/Base, Buffer, & Salt Equilibria
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Arhenius, Bronsted-Lowry, & Lewis Acids & Bases
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Strong Acids
Strong Bases
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Acid rxns
Base rxns
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A/B Equilibrium Constants
KW, KA, KB, & pH
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Calculate pH of:0.025 M HNO30.020 M KOH
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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
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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
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The take-home portion of the test is due by 8:15 tomorrow