Chapter 10. Acids, Bases, And Salts Chapter 10 Table Of .
5/10/2017Chapter 10Chapter 10. Acids, Bases, and SaltsTable of ContentsIntroduction to Inorganic ChemistryInstructor Dr. Upali Siriwardane (Ph.D. Ohio State)E-mail: upali@latech.eduOffice: 311 Carson Taylor Hall ; Phone: 318-257-4941;Office Hours: MWF 8:00-9:00 and 11:00-12:00;TR 10:00-12:00Contact me trough phone or e-mail if you have questionsOnline Tests on Following daysMarch 24, 2017: Test 1 (Chapters 1-3)April 10, 2017 :Test 2 (Chapters 4-5)May 1, 2017: Test 3 (Chapters 6,7 &8)May 12, 2017 : Test 4 (Chapters 9, 10 &11)May 15, 2017: Make Up Exam: Chapters 1110.1210.1310.1410.1510.16Arrhenius Acid-Base TheoryBrønsted-Lowry Acid-Base TheoryMono-, Di-, and Triprotic AcidsStrengths of Acids and BasesIonization Constants for Acids and BasesSaltsAcid-Base Neutralization ReactionsSelf-Ionization of WaterThe pH ConceptThe pKa Method for Expressing Acid StrengthThe pH of Aqueous Salt SolutionsBuffersThe Henderson-Hasselbalch EquationElectrolytesEquivalents and Milliequivalents of ElectrolytesAcid-Base TitrationsCopyright Cengage Learning. All rights reservedSection 10.1Section 10.1Arrhenius Acid-Base TheoryArrhenius Acid-Base Theory2Ionization Arrhenius acid: hydrogen-containing compoundthat produces H ions in solution. Example: HNO3 H NO3– Arrhenius base: hydroxide-containing compoundthat produces OH– ions in solution. Example: NaOH Na OH–Copyright Cengage Learning. All rights reserved The process in which individual positive andnegative ions are produced from a molecularcompound that is dissolved in solution.– Arrhenius acids– Example: HCl H Cl–3Copyright Cengage Learning. All rights reservedSection 10.1Section 10.1Arrhenius Acid-Base TheoryArrhenius Acid-Base TheoryDissociationDifference Between Ionization and Dissociation4 The process in which individual positive andnegative ions are released from an ioniccompound that is dissolved in solution.– Arrhenius Bases– Example: KOH K OH–Copyright Cengage Learning. All rights reserved5Copyright Cengage Learning. All rights reserved61
5/10/2017Section 10.2Section 10.2Brønsted-Lowry Acid-Base TheoryBrønsted-Lowry Acid-Base TheoryBrønsted-Lowry Reaction Brønsted-Lowry acid: substance that can donatea proton (H ion) to some other substance;proton donor. Brønsted-Lowry base: substance that canaccept a proton (H ion) from some othersubstance; proton acceptor.HCl H2O Cl H3O acid baseTo play movie you must be in Slide Show ModePC Users: Please wait for content to load, then click to playMac Users: CLICK HERECopyright Cengage Learning. All rights reserved7Copyright Cengage Learning. All rights reserved8Section 10.2Section 10.2Brønsted-Lowry Acid-Base TheoryBrønsted-Lowry Acid-Base TheoryAcid in WaterAcid dissociation EquilibriumH3 O(aq) C2H3O2-(aq)HC2H3O2(aq) H2O(l)HA(aq) acidH3O (aq) Copyright Cengage Learning. All rights reserved9Ka [H ][C2H3O2-]-----------------[HC2H3O2]Copyright Cengage Learning. All rights reservedSection 10.2Section 10.2Brønsted-Lowry Acid-Base TheoryBrønsted-Lowry Acid-Base TheoryBase dissociation EquilibriumAcid Ionization EquilibriumNH3(aq) H2O(l)NH3;Kb 10NH4 (aq) OH-(aq)[NH4 ][OH-]-----------------[NH3]To play movie you must be in Slide Show ModePC Users: Please wait for content to load, then click to playMac Users: CLICK HERECopyright Cengage Learning. All rights reserved11Copyright Cengage Learning. All rights reserved122
5/10/2017Section 10.2Section 10.3Brønsted-Lowry Acid-Base TheoryMono-, Di-, and Triprotic AcidsAmphiprotic SubstanceMonoprotic Acid A substance that can either lose or accept aproton and thus can function as either aBrønsted-Lowry acid or a Brønsted-Lowry base. Example: H2O, H3O H2O, OH– An acid that supplies one proton (H ion) permolecule during an acid-base reaction.Copyright Cengage Learning. All rights reservedHA H2O13A H3O Copyright Cengage Learning. All rights reserved14Section 10.3Section 10.3Mono-, Di-, and Triprotic AcidsMono-, Di-, and Triprotic AcidsDiprotic AcidTriprotic Acid An acid that supplies two protons (H ions) permolecule during an acid-base reaction. An acid that supplies three protons (H ions) permolecule during an acid-base reaction.H 2 A H2 OHA H2OHA H3O ; Ka1A2 H3O ; Ka2Copyright Cengage Learning. All rights reservedH 3 A H2 OH2A H2OHA2 H2O15H2A H3O ; Ka1HA2 H3O ; Ka2A3 H3O ; Ka3Copyright Cengage Learning. All rights reservedSection 10.3Section 10.4Mono-, Di-, and Triprotic AcidsStrengths of Acids and BasesPolyprotic AcidDifferences Between Strong and Weak Acids in Terms of SpeciesPresent16 An acid that supplies two or more protons (H ions) during an acid-base reaction. Includes both diprotic and triprotic acids.Copyright Cengage Learning. All rights reserved17Copyright Cengage Learning. All rights reserved183
5/10/2017Section 10.4Section 10.4Strengths of Acids and BasesStrengths of Acids and BasesStrong AcidCommonly Encountered Strong Acids Transfers 100% of its protons to water in anaqueous solution. (aq)HCl H2O H3O (aq) Cl (aq) Ionization equilibrium lies far to the right (product). Yields a weak conjugate base Cl- ion .Copyright Cengage Learning. All rights reserved19Copyright Cengage Learning. All rights reservedSection 10.4Section 10.4Strengths of Acids and BasesStrengths of Acids and BasesWeak AcidBases Transfers small % of its protons to water in anaqueous solution.HC2H3O2(aq) H2O(l)H3 O(aq) C2H3O2-(aq)weak Acidconjugate base Ionization equilibrium lies far to the left (reactant). Yields a strong conjugate base C2H3O2- ion .Copyright Cengage Learning. All rights reserved Strong bases: hydroxides of Groups IA and IIA.21Copyright Cengage Learning. All rights reservedSection 10.5Section 10.5Ionization Constants for Acids and BasesIonization Constants for Acids and BasesAcid Ionization ConstantAcid Strength, % Ionization, and Ka Magnitude The equilibrium constant for the reaction of aweak acid with water. Acid strength increases as % ionizationincreases. Acid strength increases as the magnitude of Kaincreases. % Ionization increases as the magnitude of Kaincreases.HA(aq) H2O(l)H3O (aq) A-(aq)éH3O ùû éë A - ùûKa ë[HA ]Copyright Cengage Learning. All rights reserved2023Copyright Cengage Learning. All rights reserved22244
5/10/2017Section 10.5Section 10.6Ionization Constants for Acids and BasesSaltsBase Ionization Constant The equilibrium constant for the reaction of aweak base with water.B(aq) H2O(l) Ionic compounds containing a metal orpolyatomic ion as the positive ion and anonmetal or polyatomic ion (except hydroxide)as the negative ion. x NaCl, NH4Cl, NaSO4 NaOH All common soluble salts are completelydissociated into ions in aqueous solution.NaCl H2O(l) Na (aq) Cl (aq),BH (aq) OH–(aq)éBH ùû éëOH- ùûKb ë[B]Copyright Cengage Learning. All rights reserved25Copyright Cengage Learning. All rights reservedSection 10.7Section 10.7Acid-Base Neutralization ReactionsAcid-Base Neutralization ReactionsNeutralization ReactionFormation of Water26 The chemical reaction between an acid and ahydroxide base in which a salt and water are theproducts.Acid Base Salt waterHCl NaOH NaCl H2OH2SO4 2 KOH K2SO4 2 H2OCopyright Cengage Learning. All rights reserved27Copyright Cengage Learning. All rights reservedSection 10.8Section 10.8Self-Ionization of WaterSelf-Ionization of WaterSelf-Ionization (Auto-Ionization)Self-Ionization of Water28 Water molecules in pure water interact with oneanother to form ions.[H3O ] 1x 10-7 1x 10-7H2O H2OH3O OH– Net effect is the formation of equal amounts ofhydronium and hydroxide ions.Ionic Product H2O; Kw [H3O ][OH–] 1.00 10–14Copyright Cengage Learning. All rights reserved29Copyright Cengage Learning. All rights reserved305
5/10/2017Section 10.8Section 10.8Self-Ionization of WaterSelf-Ionization of WaterIon Product Constant for WaterRelationship Between [H3O ] and [OH–] At 24 C:Kw [H3O ][OH–] 1.00 10–14 No matter what the solution contains, theproduct of [H3O ] and [OH–] must always equal1.00 10–14.Copyright Cengage Learning. All rights reserved31Copyright Cengage Learning. All rights reservedSection 10.8Section 10.8Self-Ionization of WaterSelf-Ionization of WaterExerciseThree Possible Situations[OH–]; [H3 neutral solution [H3O ] [OH–]; acidic solution [H3O ] [OH–]; basic solutionO ]32Calculate [H3O ] or [OH–] as required for eachof the following solutions at 24 C, and statewhether the solution is neutral, acidic, or basic.a) 1.0 10–4 M OH–b) 2.0 M H3O Copyright Cengage Learning. All rights reserved33Copyright Cengage Learning. All rights reservedSection 10.8Section 10.9Self-Ionization of WaterThe pH Concept34Exercise Calculate [H3O ] or [OH–] as required for eachof the following solutions at 24 C, and statewhether the solution is neutral, acidic, or basic.a) 1.0 10–4 M OH–pH –log[H3O ]A compact way to represent solution acidity.pH decreases as [H ] increases.pH range between 0 to 14 in aqueous solutionsat 24 C.1.0 10–10 M H3O ; basicb) 2.0 M H3O 5.0 10–15 M OH–; acidicCopyright Cengage Learning. All rights reserved35Copyright Cengage Learning. All rights reserved366
5/10/2017Section 10.9Section 10.9The pH ConceptThe pH ConceptExerciseExerciseCalculate the pH for each of the followingsolutions.Calculate the pH for each of the followingsolutions.a) 1.0 10–4 M H3O a) 1.0 10–4 M H3O b)0.040 M OH–b)0.040 M OH–pH 4.00pH 12.60Copyright Cengage Learning. All rights reserved37Copyright Cengage Learning. All rights reservedSection 10.9Section 10.9The pH ConceptThe pH ConceptExerciseExerciseThe pH of a solution is 5.85. What is the [H3O ]for this solution?The pH of a solution is 5.85. What is the [H3O ]for this solution?38[H3O ] 1.4 10–6 MCopyright Cengage Learning. All rights reserved39Copyright Cengage Learning. All rights reservedSection 10.9Section 10.9The pH ConceptThe pH Concept40pH Range pH 7; neutral pH 7; basic– Higher the pH, more basic. pH 7; acidic– Lower the pH, more acidic.Copyright Cengage Learning. All rights reservedRelationships Among pHValues, [H3O ], and [OH–]41Copyright Cengage Learning. All rights reserved427
5/10/2017Section 10.10Section 10.10The pKa Method for Expressing Acid StrengthThe pKa Method for Expressing Acid StrengthExercise pKa –log Ka pKa is calculated from Ka in exactly the sameway that pH is calculated from [H3O ].Copyright Cengage Learning. All rights reservedCalculate the pKa for HF given that the Kafor this acid is 6.8 10–4.43Copyright Cengage Learning. All rights reservedSection 10.10Section 10.11The pKa Method for Expressing Acid StrengthThe pH of Aqueous Salt SolutionsExercise44Salts Ionic compounds. When dissolved in water, break up into its ions(which can behave as acids or bases). Hydrolysis – the reaction of a salt ions with water toproduce hydronium ion or hydroxide ion or both. NH4 Cl NH4 Conjugate acid of weak base NH4 H2O NH3 H3O Calculate the pKa for HF given that the Kafor this acid is 6.8 10–4.pKa 3.17aCopyright Cengage Learning. All rights reserved45Copyright Cengage Learning. All rights reservedSection 10.11Section 10.11The pH of Aqueous Salt SolutionsThe pH of Aqueous Salt SolutionsTypes of Salt HydrolysisTypes of Salt Hydrolysis1. The salt of a strong acid and a strong base doesnot hydrolyze, so the solution is neutral. KCl, NaNO32. The salt of a strong acid and a weak basehydrolyzes to produce an acidic solution. NH4Cl46NH4 H2O NH3 H3O Copyright Cengage Learning. All rights reserved47Copyright Cengage Learning. All rights reserved488
5/10/2017Section 10.11Section 10.11The pH of Aqueous Salt SolutionsThe pH of Aqueous Salt SolutionsTypes of Salt HydrolysisTypes of Salt Hydrolysis3. The salt of a weak acid and a strong basehydrolyzes to produce a basic solution. NaF,F– H2O HF OH–F– Conjugate base of weak acid KC2H3O2C2H3O2– H2O HC2H3O2 OH–C2H3O2– Conjugate acid of weak acid4. The salt of a weak acid and a weak basehydrolyzes to produce a slightly acidic, neutral,or slightly basic solution, depending on therelative weaknesses of the acid and base.Copyright Cengage Learning. All rights reserved49Copyright Cengage Learning. All rights reservedSection 10.11Section 10.11The pH of Aqueous Salt SolutionsThe pH of Aqueous Salt SolutionsNeutralization “Parentage” of SaltsNeutralization “Parentage” of SaltsCopyright Cengage Learning. All rights reserved51Section 10.11The pH of Aqueous Salt SolutionsWhat salt solutions would be acidic, basic and neutral?1)2)3)4)strong acid strong base neutralweak acid strong base basicstrong acid weak base acidicweak acid weak base neutral,basic or an acidic solution dependingon the relative strengths of the acid andthe base.Copyright Cengage Learning. All rights reserved5052Section 10.12BuffersKey Points about Buffers Buffer – an aqueous solution containingsubstances that prevent major changes insolution pH when small amounts of acid or baseare added to it. They are weak acids or bases containing acommon ion. Typically, a buffer system is composed of aweak acid and its conjugate base.Copyright Cengage Learning. All rights reserved549
5/10/2017Section 10.12Section 10.12BuffersBuffersBuffers Contain Two Active Chemical SpeciesAdding an Acid to a Buffer1. A substance to react with and remove addedbase.2. A substance to react with and remove addedacid.To play movie you must be in Slide Show ModePC Users: Please wait for content to load, then click to playMac Users: CLICK HERECopyright Cengage Learning. All rights reserved55Copyright Cengage Learning. All rights reservedSection 10.12Section 10.12BuffersBuffersBuffersAddition of Base [OH– ion] to the BufferHA H2OH3O A–– The added OH ion reacts with H3O ion,producing water (neutralization). The neutralization reaction produces the stressof not enough H3O ion because H3O ion wasconsumed in the neutralization. The equilibrium shifts to the right to producemore H3O ion, which maintains the pH close toits original level.To play movie you must be in Slide Show ModePC Users: Please wait for content to load, then click to playMac Users: CLICK HERECopyright Cengage Learning. All rights reserved57Section 10.1258The Henderson-Hasselbalch EquationO ion] to the BufferHenderson-Hasselbalch EquationHA H2OH3O A– The added H3O ion increases the overallamount of H3O ion present. The stress on the system is too much H3O ion. The equilibrium shifts to the left consuming mostof the excess H3O ion and resulting in a pHclose to the original level.Copyright Cengage Learning. All rights reservedCopyright Cengage Learning. All rights reservedSection 10.13BuffersAddition of Acid [H356éA- ùpH pK a log ë û[HA ]59Copyright Cengage Learning. All rights reserved6010
5/10/2017Section 10.13Section 10.14The Henderson-Hasselbalch EquationElectrolytesExercise Acids, bases, and soluble salts all produce ionsin solution, thus they all produce solutions thatconduct electricity. Electrolyte – substance whose aqueous solutionconducts electricity.What is the pH of a buffer solution that is 0.45M acetic acid (HC2H3O2) and 0.85 M sodiumacetate (NaC2H3O2)? The Ka for acetic acid is1.8 10–5.pH 5.02Copyright Cengage Learning. All rights reserved61Copyright Cengage Learning. All rights reservedSection 10.14Section 10.14ElectrolytesElectrolytesNonelectrolyte – does not conduct electricityStrong Electrolyte – completely ionizes/dissociates Example: table sugar (sucrose), glucose Example: strong acids, bases, and soluble saltsCopyright Cengage Learning. All rights reserved63Copyright Cengage Learning. All rights reservedSection 10.14Section 10.15ElectrolytesEquivalents and Milliequivalents of ElectrolytesWeak Electrolyte – incompletely ionizes/dissociatesEquivalent (Eq) of an Ion Example: weak acids and bases The molar amount of that ion needed to supplyone mole of positive or negative charge.62641 mole K 1 equivalent1 mole Mg2 2 equivalents1 mole PO43– 3 equivalentsCopyright Cengage Learning. All rights reserved65Copyright Cengage Learning. All rights reserved6611
5/10/2017Section 10.15Section 10.15Equivalents and Milliequivalents of ElectrolytesEquivalents and Milliequivalents of ElectrolytesMilliequivalentConcentrations of Major Electrolytes in Blood Plasma1 milliequivalent 10–3 equivalentCopyright Cengage Learning. All rights reserved67Copyright Cengage Learning. All rights reserved68Section 10.15Section 10.15Equivalents and Milliequivalents of ElectrolytesEquivalents and Milliequivalents of ElectrolytesExerciseExerciseThe concentration of Ca2 ion present in asample is 5.3 mEq/L. How many milligramsof Ca2 ion are present in 180.0 mL of thesample?The concentration of Ca2 ion present in asample is 5.3 mEq/L. How many milligramsof Ca2 ion are present in 180.0 mL of thesample?19 mg Ca2 ion(180 mL )Copyright Cengage Learning. All rights reserved69( )( )( )(1L5.3 mEq1Eq1 mol Ca1000 mL1L1000 mEq2 Eq CaCopyright Cengage Learning. All rights reservedSection 10.16Section 10.16Acid-Base TitrationsAcid-Base Titrations2 2 )(40.08 g Ca1 mol Ca2 2 )( )1000 mg 19 mg Ca2 ion1g70Titration Setup A neutralization reaction in which a measuredvolume of an acid or a base of knownconcentration is completely reacted with ameasured volume of a base or an acid ofunknown concentration. For a strong acid and base reaction:H (aq) OH–(aq) H2O(l)Copyright Cengage Learning. All rights reserved71Copyright Cengage Learning. All rights reserved7212
5/10/2017Section 10.16Section 10.16Acid-Base TitrationsAcid-Base TitrationsAcid-Base IndicatorIndicator – yellow in acidic solution; red in basic solution A compound that exhibits different colorsdepending on the pH of its solution. An indicator is selected that changes color ata pH that corresponds as nearly as possibleto the pH of the solution when the titration iscomplete.Copyright Cengage Learning. All rights reserved73Copyright Cengage Learning. All rights reservedSection 10.16Section 10.16Acid-Base TitrationsAcid-Base TitrationsConcept Check74Concept CheckFor the titration of sulfuric acid (H2SO4) withsodium hydroxide (NaOH), how many moles ofsodium hydroxide would be required to reactwith 1.00 L of 0.500 M sulfuric acid to reach theendpoint?For the titration of sulfuric acid (H2SO4) withsodium hydroxide (NaOH), how many moles ofsodium hydroxide would be required to reactwith 1.00 L of 0.500 M sulfuric acid to reach theendpoint?H2SO4 2NaOH Na2SO4 2 H2O1.00 mol NaOHCopyright Cengage Learning. All rights reserved75Copyright Cengage Learning. All rights reserved7613
10.3 Mono-, Di-, and Triprotic Acids 10.4 Strengths of Acids and Bases 10.5 Ionization Constants for Acids and Bases 10.6 Salts 10.7 Acid-Base Neutralization Reactions 10.8 Self-Ionization of Water 10.9 The pH Concept 10.10 The pKa Method for Expressing Acid Strength 10.11 The pH
2. Describe the common properties of acids and bases 3. Identify acids and bases using indicators, pH papers 4. Name some common lab acids and bases, acids at and bases at home 5. Describe reactions of acids with metals, bases and carbonates 6. Describe the application of acids, bases and p
_7. Which statement describes an alternate theory of acids and bases? (1) Acids and bases are both H acceptors. (2) Acids and bases are both H donors. (3) Acids are H acceptors, and bases are H donors. (4) Acids are H donors, and bases are H acceptors. _8. Which substance is the
Properties of Acids and Bases Return to the Table of contents Slide 5 / 208 What is an Acid? Acids release hydrogen ions into solutions Acids neutralize bases in a neutralization reaction. Acids corrode active metals. Acids turn blue litmus to red. Acids taste sour. Properties of Acids Slide 6 / 208 Properties
Lecture Notes for Chapter 16: Acids and Bases I. Acids and Bases a. There are several ways to define acids and bases. Perhaps the easiest way to start is to list some of the properties of acids and bases. b. The table below summarizes some properties that will be helpful
Acids, Bases, and pH The hydrohalic acids (HX (aq)), where X represents a halogen) include HF, HCl, HBr, and HI. Only HF is a weak acid. The rest are strong acids. What factors account for this difference? 8.1 Explaining the Properties of Acids and Bases 8.2 The Equilibrium of Weak Acids and Bases 8.3
properties of acids and bases. 5. Describe the colors that form in acidic and basic solutions with litmus paper and phenolphthalein. 6. Explain the difference between strong acids or bases and weak acids or bases. 7. Memorize the strong acids and bases. 8. Define the terms polyprotic and amphiprotic. 9. Perform calculations using the following .
Unit 12 Acids and Bases- Funsheets Part A: Name and write the formula for the following acids and bases. 1) Carbonic acid _ . Part E: Using your knowledge of acids and bases, answer the following questions. 1) Fill in the following Venn diagram about properties of acids and bases. You must fill in at least 4 facts in each.
Unit 11 Objectives: Acids & Bases Acid-Base Nomenclature Content Objectives: I can name ionic compounds containing acids, and bases, using (IUPAC) nomenclature rules. I can write the chemical formulas of acids and bases. Criteria for Success: I can identify an acid as a binary acid or an oxyacid. I can name common binary acids, oxyacids, and bases given their chemical formula.
