Chapter 5 Acid-Base Equilibrium X 5.1 The Bronsted theory of acids and bases ק5.2 Ionization equilibrium of water and the pH scale X$5.3 Equilibrium in solutions of weak acids and weak bases X 5.4 Buffer solutions
Chapter 5 Acid-Base Equilibrium § 5.4 Buffer solutions § 5.3 Equilibrium in solutions of weak acids and weak bases § 5.2 Ionization equilibrium of water and the pH scale § 5.1 The Brønsted theory of acids and bases
5.5 Acid-bases indicators X 5.6 Lewis acids and bases and coordination compounds X 5.7 Complexation reaction and coordination equilibrium
§ 5.7 Complexation reaction and coordination equilibrium § 5.6 Lewis acids and bases and coordination compounds § 5.5 Acid-bases indicators
5.1 The Bronsted theory of acids and bases 5.1.1 The Bronsted acids and bases 5.1.2 Relative strengths of acids and bases
§ 5.1 The Brønsted theory of acids and bases 5.1.2 Relative strengths of acids and bases 5.1.1 The Brønsted acids and bases
Overview:(sour,bitter)Taste-→Arrhenius theory(酸碱电离理论， Ht&OH),→Solvent theory,Bronsted theory(质子理论)，Lewis theory(电子理论)，soft-hard acid/base theory. 5.1.1 The Bronsted theory of acids and bases(酸碱质子理论) acid:a substance capable of donating a proton.(proton donor) (质子的给予体) base:a substance that can accept a proton.(proton acceptor) (质子的接受体)
acid: a substance capable of donating a proton. (proton donor) （质子的给予体） base: a substance that can accept a proton. (proton acceptor) （质子的接受体） 5.1.1 The Brønsted theory of acids and bases (酸碱质子理论） Overview: (sour, bitter) Taste Arrhenius theory(酸碱电离理论, H+&OH- ), Solvent theory, Bronsted theory(质子理论), Lewis theory(电子理论), soft-hard acid/base theory…
an acid -H+a base HAc =H*+Ac H2PO-H*+HPO2 HPO子=H*+PO NH-H*+NH3 [CH:NH3]*=H*+CH:NH2 [Fe(H2O)]*-H*+[Fe(OH)(H2O);]2* [Fe(OH)(H2O)]2*-H*+[Fe(OH)2(H2O)T conjugate acid conjugate base an acid-base conjugate pair(共轭酸碱对)
an acid H+ + a base + - HAc H + Ac - + - + 2 H2PO 4 H HPO 4 - + - + 3 4 2 HPO 4 H PO + + + NH 4 H NH 3 [ ] + + + CH 3NH 3 H CH 3NH 2 + + + + 2 2 5 3 [Fe(H 2O) 6 ] H [Fe(OH)(H O) ] + + + + 2 2 4 2 [Fe(OH)(H 2O) 5 ] H [Fe(OH) (H O) ] conjugate acid conjugate base an acid-base conjugate pair (共轭酸碱对)
amphiprotic substance(两性物质)： a substance that can either donate or accept a proton is said to be amphiprotic. Example:HSO,[Fe(OH)(H2O)s]2,HCO3,H2O,HS-etc the essence of acid-base reaction in Bronsted theory is proton transfer between two acid-base conjugate pairs,examples are given below:
amphiprotic substance(两性物质)： a substance that can either donate or accept a proton is said to be amphiprotic. HCO3 - , H2O, HS- [Fe(OH)(H etc 2O)5 ] 2+ HSO , 4 - Example: , the essence of acid-base reaction in Brønsted theory is proton transfer between two acid-base conjugate pairs, examples are given below:
DThe ionization reactions of acids and bases in solvent are proton-transfer reactions. Example:the ionization of HF in water can be represented as HF(aq)-H++F(aq) H++H2O(1)-H3O*(aq) HF(aq)+H2O(1)=H3O*(aq)+F(aq) 2Water is an amphiprotic substance,its autoionization is also proton-transfer reaction. H中 H2O(I)+H2O(I)-H3O*(aq)+OH-(aq) acid(1) base(2) acid(2) base(1)
① The ionization reactions of acids and bases in solvent are proton-transfer reactions. Example: the ionization of HF in water can be represented as ② Water is an amphiprotic substance, its autoionization is also proton-transfer reaction. H+ acid(1) base(2) acid(2) base(1) HF(aq) H+ + F－(aq) H+ + H2O(l) H3O+ (aq) HF(aq) + H2O(l) H3O+ (aq) + F－(aq) H2O(l)+H2O(l) H3O+ (aq) +OH－(aq)
③The hydrolysis of salts(no“salt”term in Bronsted theory)can be regarded as proton-transfer reactions of acids and bases.Example:the hydrolysis of NaAc H中 AC-+H,O÷OH-+HAc base(1)acid(2) base(2)acid(1) the hydrolysis of NHCl: H+ NH +H2O-H2O++NH; acid(1)base(2) acid(2) base(1)
③ The hydrolysis of salts (no ―salt‖ term in Brønsted theory) can be regarded as proton-transfer reactions of acids and bases. Example: the hydrolysis of NaAc base(1) acid(2) base(2) acid(1) H+ the hydrolysis of NH4Cl： acid(1) base(2) acid(2) base(1) H+ Ac－+H2O OH－ + HAc + H2O H3O+ + NH3 + NH4
4 The acid-base reactions in non-aqueous solution can also be regarded as proton-transfer reactions.Example: the formation reaction of NHCl: H+ HCI NH- NH acid(1) base(2) acid(2) base(1) the neutralization reaction in liquid ammonia H NH CI+NaNH 2NH+NaCl acid(1) base(2) acid(2)+base(1)
④ The acid-base reactions in non-aqueous solution can also be regarded as proton-transfer reactions. Example: the formation reaction of NH4Cl： H+ the neutralization reaction in liquid ammonia ： H+ + - HCl + NH NH + Cl 3 4 NH Cl NaNH 2NH NaCl 4 + 2 3 + acid(1) base(2) acid(2) base(1) acid(1) base(2) acid(2)+ base(1)
5.1.2 Relative strengths of acids and bases The strength of an acid or a base refers to the ability of donating proton for an acid or accepting proton for a base. HAc HCN HCI,HNO3 K3 1.8×10-5 5.8×10-10 H-Cl: differentiating effect(区分效应)： e.g.:H2O can differentiate the relative strength of HAc,HCN leveling effect((拉平效应)：a solvent's ability to level the effect of a strong acid or base dissolved in it
HAc HCN differentiating effect(区分效应)： e.g.：H2O can differentiate the relative strength of HAc，HCN. leveling effect(拉平效应)：a solvent's ability to level the effect of a strong acid or base dissolved in it. The strength of an acid or a base refers to the ability of donating proton for an acid or accepting proton for a base. 5.1.2 Relative strengths of acids and bases 1.8×10 K -5 a 5.8×10-10 HCl， HNO3