Chapter 16 Overview: •Definitions Arrhenius Bronsted -- Conjugate Pairs Hydronium Ion •Relative Strengths Strong/Weak acids and reactions Strong/Weak bases and reactions Ka’s and Kb’s •pH and H2O Ionization •Calculating Equilibrium Concentrations •Hydrolysis Acidic and Basic Salts •Polyprotic Acids •Molecular Structure/Bonding •Lewis Acids and Bases Acids •sour •corrosive •reddens blue vegetable colors •react with bases Bases •bitter •soapy •restores vegetable colors reddened by acids •react with acids Arrhenius Acid: substance that releases or produces H+ HCl(aq) H+(aq) + Cl -(aq) Arrhenius Base: substance that releases or produces OH NaOH(aq) Na+(aq) + OH -(aq) Bronsted Acid: substance that donates a H+ to another HNO3(aq) + H2O(l) H3O+(aq) + NO3-(aq) Bronsted Base: substance that accepts a H+ from another CO32-(aq) + H2O(l) HCO3-(aq) + OH -(aq) Water Dissociation: 2H2O H3O+ + OH - Hydronium Ion -- because bare protons are unlikely d+ O H H d- O H H H+ transfer - O +H O H H H + pH and Water Ionization: 2H2O(l) H3O+(aq) + OH -(aq) K = [H3O+][OH -] = K [H2O]2 = [H3O+][OH -] [H2O] 2 Kw = [H3O+][OH -] = 1.0 x 10 -14 (at 25C) Reactant Favored ion-product constant for water pH = - log [H+] = - log [H3O+] neutral solution: 2H2O [H3O+] = [OH -] H3O+ + OH - 1.0 x 10 -14 = [H3O+][OH -] = [H3O+]2 [H3O+] = 1.0 x 10 -7 M pH = - log (1.0 x 10 -7) = 7.0 non-neutral solutions: acidic solutions: [H+] > [OH-] pH < 7.0 basic solutions: [H+] < [OH-] pH > 7.0 pH of Strong Acid and Base Solutions: Calculate the pH of a solution containing 0.00100 M of a strong acid such as HCl. HCl(aq) 0.00100 H+(aq) + OH-(aq) 0.00100 0.00100 pH = - log (0.00100) = 3.00 but. . . . What about H3O+ from water? 2 H2O initial change equil. H3O+ + 0.00100 OH 0 +x +x 0.00100 + x x 1 x 10 -14 = (0.00100 + x)(x) x = H3O+ and OH- from disso. of water Kw = [H3O+] [OH -] 0 x is very small compared to 0.00100 & can be neglected 1 x 10 -14 = (0.00100 + x)(x) x = 1.00 x 10 -11 M = [OH -] pOH = 11.0 [H+] [H3O+] [H3O+] (1.0 x 10-11) = 1.0 x 10 -14 [H3O+] = 1.0 x 10 -3 M the conc. of H+ in a solution of a strong acid is the conc. of the strong acid pH = 3.0 Note: pH + pOH = 14.0 Bottom Line: [H+] = [H3O+] = [H5O2+] = [H9O4+] hydrated hydrogen ions neutral solution [H3O+] = [OH-] pH = 7 acidic solution [H3O+] > [OH-] pH < 7 basic solution [H3O+] < [OH-] pH > 7 the concentration of [H3O+] in a strong acid is the concentration of the acid Calculate the pH of a solution containing 0.010 M KOH. KOH 0.010 M K+(aq) + 0.010 M OH-(aq) 0.010 M strong base, complete rxn, stoichiometric 1.0 x 10 -14 = [H+] (0.010 M) [H+] = 1.0 x 10 -12 M pH = 12.0 contribution of [H+] from dissociation of H2O is negligible Calculate the [H+] and [OH -] in a solution that has a pH = 8.60 - log [H+] = pH - log [H+] = 8.60 log [H+] = -8.60 [H+] = anti log (-8.60) [H+] = 1.8 x 10 -4 M [OH -] = 5.6 x 10 -11 M pH 14 [H3O+] 10 -14 [OH-] 1 pOH 0 Basic ammonia human blood milk 7.0 10 -7 10 -7 7.0 vinegar, cola 0 1 10 -14 14 Neutral Acidic Measuring pH: pH meter -- electrodes measure pH – most precise method acid-base indicators – less precise but good when a pH meter is not available – substances which are differently colored at different pH values – litmus, phenolphthalein, thymol blue Arrhenius Acid: substance that releases or produces H+ HCl(aq) H+(aq) + Cl -(aq) Arrhenius Base: substance that releases or produces OH NaOH(aq) Na+(aq) + OH -(aq) Bronsted Acid: substance that donates a H+ to another HNO3(aq) + H2O(l) H3O+(aq) + NO3-(aq) Bronsted Base: substance that accepts a H+ from another CO32-(aq) + H2O(l) HCO3-(aq) + OH -(aq) Examples: H+ NH4+(aq) + H2O(l) H3O+(aq) + NH3(aq) acid base H+ conjugate acid conjugate base conjugate pair PO43-(aq) + H2O(l) HPO42-(aq) + OH -(aq) base acid conjugate acid conjugate base conjugate pair Some species can act as an acid or base: H+ HCO3-(aq) + H2O(l) acid H3O+(aq) + CO32-(aq) conjugate acid base conjugate base H+ HCO3-(aq) + H2O(l) base acid H2CO3(aq) + OH -(aq) conjugate acid conjugate base HCO3- is an amphiprotic substance You Must Know: what an acid and a base is and how to identify both know definitions and properties the reaction of an acid and a base with water how to identify acid, base, conjugate acid and conjugate base what the hydronium ion is and the ionization reaction of water Problems: HX + H2O H3O+ + X A B CA •What is the conjugate base of: H2S NH4+ NH3 H2O OH - HS NH3 NH2OH O2- •What is the conjugate acid of: NO3HNO3 HPO42H2PO4H3SO4+ H2SO4 CB Relative Strengths: HCl + stronger A H2O stronger B H3O+ + Cl - weaker A weaker B equilibrium is a competition between the bases H2O and Cl - -- the equilibrium will lie toward the direction of the weaker acid and base in this case, H2O is a stronger base than Cl - as it competes much more effectively for the H+ HCN + weaker A H2O weaker B H3O+ + CN stronger A H2O < CN - stronger B Which is the weaker acid: H2S + CN - HCN + HS - HCN HCO3- + SO42- HSO4- + CO32- HCO3- HClO4 + H2O H3O+ + ClO4- H3O+ NH4+ + H3O+ + NH3 NH4+ H 2O The stronger the acid the weaker its conjugate base: strongest acid weakest acid weakest conjugate base strongest conjugate base Given the following, which is the weaker conjugate: acids bases HCl > CH3CO2H Cl - HCN < H3PO4 CN - H2SO4 > H2SO3 HSO4 NH3 > H2O NH4 HSO4- H2SO4 > HCO3 - H - > < CO32NH3 < CH3CO2- > H2PO4 - < + H2 < HSO3- < H3O+ NH4+ Predicting Direction of Acid/Base Rxns. CH3CO2H stronger A stronger B + CN - weaker B HCN + CH3CO2 - weaker A stronger A HSO4- + NH3 stronger B weaker A NH4+ + SO42- weaker B Strong Acids and Bases •Strong Acids HCl HNO3 HClO4 HClO3 H2SO4 HBr HI HX + H2O H3O+ + X - •Strong Bases Grp I hydroxides Grp II hydroxides (except Be) MOH essentially complete rxns. M+ + OH - Weak Acids and Bases: HX + H2O H3O+ + X - Ka = [H3O+][X -] [HX] B + H2O < 1 BH+ + OH - Kb = [BH+][OH -] [B] < 1 Weak Acids Can Be: •cations NH4+ or [Cu(H2O)6]2+ •anions H2PO4- or HCO3- •neutral CH3CO2H or HCO2H Weak Bases Can Be: •anions CO32- or •neutral NH3 or CN (CH3)3N You Must: Be able to determine direction of rxn based on acid or base relative strengths Know the strong acids and strong bases Be able to recognize weak acids and bases Know water ionization rxn, constant and expression Know what pH is and how to calculate it Know how to calculate equil. conc., pH, pOH for weak acids and bases Problem 1: A 0.015 M solution of an unknown base has a pH of 10.09. Is it a strong or weak base? What is the Kb, if it is weak? Problem 2: What are the equil. conc. of H3O+, acetate ion, acetic acid in a 0.20 M aqueous solution of acetic acid, CH3CO2H? Use the approximation whenever possible: When the initial weak acid/base conc. > 100 *Ka/b neglect x when it is added to or subtracted from the initial conc. Answer 1: If this were a strong base then [OH-] = 0.015 M and pOH = 1.8 and pH = 12.2. B + H2O HB+ + OH- pH = 10.09 and pOH = 3. 91 [OH-] = 1.2 x 10-4 Kb = [HB+][OH-] = (1.2 x 10 -4)2 [B] (0.015) = 9.6 x 10 -7 Answer 2: CH3CO2H + H2O initial 0.20 change -x equil. 0.20 -x H3O+ + CH3CO20 +x x 0 +x x Ka = 1.8 x 10 -5 = [H3O+][CH3CO2-] [CH3CO2H] Ka = 1.8 x 10 -5 = (x)(x) (0.20 -x) x2 = 3.6 x 10 -6 x = 1.9 x 10 -3 [CH3CO2-]=[H3O+] = 1.9 x 10 -3 M [CH3CO2H] = 0.20 M pH = 2.7 What is the percent ionization? % ion = [H3O+] x 100 [CH3CO2H] = 0.95 % Polyprotic Acids and Bases: H3PO4 + H2O H3O+ + H2PO4- Ka1 H2PO4- + H2O H3O+ + HPO42- Ka2 HPO42- + H2O H3O+ + PO43- H3PO4 + 3H2O Ka3 3H3O+ + PO43-- Ka tot = Ka1 Ka2 Ka3 (7.5 x 10 -3)(6.2 x 10 -8)(3.6 x 10 -13) = 1.7 x 10 -22 Weak Bases: Can be anions such as: – CN-, HSO3-, SO32-, HCO3-, CO32-, etc. Can be N-containing compounds, such as: – NH3, (CH3)NH2, (CH3)2NH, (CH3)3N, etc. React with water – B- + H2O HB + OH- – B + H2O HB+ + OH- or Have base dissociation constants, Kb Example: NH3 + H2O initial 0.20 M change -x equil. 0.20 -x NH4+ + OH 0 +x x 0 +x x Kb = 1.8 x 10 -5 = [NH4+][OH -] [NH3] Kb = 1.8 x 10 -5 = (x)(x) (0.20 -x) x2 = 3.6 x 10 -6 x = 1.9 x 10 -3 [NH4+]=[OH-] = 1.9 x 10 -3 M [NH3] = 0.20 M pOH = 2.7 pH = 12.3 CO3 -2 + H2O OH - + HCO3-- Kb1 HCO3 -- + H2O OH - + H2CO3 Kb2 CO3 + 2H2O 2OH -- + H2CO32-- Kb tot = Kb1 Kb2 (2.1 x 10 -4)(2.4 x 10 -8) = 5.0 x 10 -12 Relationship of an acid Ka and the Kb of its conjugate base: conjugate pair rxns with water NH3 + H2O NH4+ + NH4+ + H2O 2H2O NH3 H 3O+ + OH - Kb = 1.8 x 10 -5 + H3O+ Ka = 5.6 x 10 -10 OH - Kw = 1 x 10 -14 For Conjugate Acid/Base Pairs: K b K a = Kw or pKb + pKa = pKw Find Ka for the conjugate acids of the following bases: Ka = Kw/Kb Base Kb Conj. Acid NH3 1.8 x 10 -5 NH4+ C5H5N 1.7 x 10 -9 HS CO3 2- Ka 5.6 x 10 -10 C5H5NH + 5.9 x 10 -6 1.8 x 10 -7 H2S 5.6 x 10 -8 1.8 x 10 HCO3 - 5.6 x 10 -11 -4 Acid/Base Hydrolysis Many salts produce solutions that are acidic or basic Why? because either (or both) the cation or anion of the salt acted as a weak acid or a weak base HX + H2O H3O+ + X - weak acid or B + H2O weak base BH+ + OH - Which cations will not hydrolyze? Cations of strong bases -- Grp I and II (except Be) Li+ Na+ K+ Rb+ Cs+ Mg2+ Ca2+ Sr2+ Ba2+ Anions of strong acids -ClO4- ClO3- SO42- NO3- Cl - Br - I- All other cations and anions will hydrolyze Which cations will hydrolyze? Conjugate acids of weak bases: NH4+ Al3+ Cu2+ etc. Conjugate bases of weak acids: CO32 - CH3CO2- NH3 F - etc. What is the pH of the following salt solutions? •NaCl Na+ -- neutral Cl - -- neutral N •NaF Na+ -- neutral F - -- basic B •NH4Cl NH4+ -- acidic Cl - -- neutral A •Na2CO3 Na+ -- neutral CO32- -- basic B •Cr(NO3)3 Cr3+ -- acidic NO3- -- neutral A •KNO3 K+ -- neutral NO3+ -- neutral N •NaC3H2O4 Na+ -- neutral C3H2O4- -- basic B •NH4CH3CO2 NH4+ -- acidic CH3CO2- -- basic ? Is NH4CH3CO2 acidic or basic? NH4+ + H2O H3O+ + NH3 Ka = 5.6 x 10 -10 CH3CO2- + H2O CH3CO2H + OH - Kb = 5.6 x 10 -10 weak acid & weak base strength equal -- neutral soln. You Must: Know what hydrolysis is Know which cations hydrolyze or produce acidic solutions Know which anions hydrolyze or produce basic solutions Be able to estimate and calculate the pH of a salt solution Know how to determine Ka’s & Kb’s of conjugate pairs Strength of Acids: Can be increased by anything that facilitates the loss of a Proton (H+) •Bond Strength •Polarity or Delectronegativity •Central Atom Charge or Oxidation # IVA VA VIA VIIA row 2 CH4 NH3 H2O HF row 3 SiH4 PH3 H2S HCl Increasing acid strength Increasing acid strength Examples: HClO4 HClO3 HClO2 HClO Cl ox. # Increasing acid strength Acid Ka +7 strong +5 strong +3 1.1 x 10 -2 +1 3.0 x 10 -8 HClO HBrO HIO Ka Increasing acid strength Acid 3 x 10 -8 2.5 x 10 -9 2.3 x 10 -11 Organic Acids: H H O C C H O- H Acetate ion resonance H O- C C H O H H O C C OH H Acetic Acid Ka = 1.8 x 10 -5 F F O C C OH F Trifluoroacetic Acid Ka = 5.0 x 10 -1 Lewis Acids and Bases: Lewis Acid -- accepts a pair of electrons Lewis Base -- donates a pair of electrons formation of a coordinate covalent bond H H B N H F F F NH3 H H Lewis Base -donates a pair of electrons + H+ H+ N H NH4 + Lewis Acid -accepts a pair of electrons