To know essential points of the Bronsted theory of acids and bases and basic concepts on the theory about Lewis acids and bases.To master ionization of water. standard ion-product constant of water,and calculation of pH of strong acid and strong base.To master the ionization equilibria of monoprotic weak acid and weak base,the calculation of equilibrium composition;to be familiar with equilibrium of stepwise process of polyprotic weak acid and calculation of equilibrium composition. To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base,and salt of monoprotic weak bases and strong acid,calculation of equilibrium composition,to be familiar with multi-step hydrolysis of salt of polyprotic weak acid and calculation of equilibrium composition.To master the concepts of common ion effect and buffer solution,and calculation of pH of a buffer solution.To master the basic concepts on complex,to know how to name a complex,To master complex formation reaction and its equilibrium,to know calculation of equilibrium composition,to know calculation of equilibrium composition under the condition of coexistence of equilibrium of acid and base reaction and dissociation equilibrium of complex. important and difficult points: Essential points of the Bronsted theory of acids and bases:concepts of acid,base,amphiprotic substance;conjugate acid-base pair.The essential of acid-base reaction is transfer of protons.The essential of ionization of water,ionization of acid and base,as well as that hydrolysis of salt are transfer of protons.The major content on Lewis acids and bases:the concept of Lewis acids and bases.The ligand in a complex is Lewis base.lonization equilibrium of water:ion- product constant of water,influence of temperature on ion-product constant of water,T=298K.Kw(298K)=1.0x1014 PH=-Igc(H+))POH=- lg'c(OH-)1,298K,PH+POH=14.00.Of importance is to master the ionization equilibrium in solutions of monoprotic weak acids and weak bases,ionization equilibrium constant,percent ionizaton(),calculation of equilibrium composition and pH of a reaction,the conditions for approximate calculation and methods of calculation.To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base,and salt of monoprotic weak bases and strong acid,the relationship between constant of ionization of water and constant of ionization of acid and base.Features of salt of polyprotic weak acids:multi-steps hydrolysis;relationship between ionization constant and hydrolysis constant,simple calculation of hydrolysis equilibrium of salt of polyprotic weak aicd and strong base(treat it as an equilibrium of hydrolysis of polyprotic base). To be familiar with concepts of ligand,coordination atom,coordination number etc about coordination compound,naming normal compounds,distinguish simple and chelating complexes,ie,normal ligands.The dissociation equilibrium of complex(stepwise process),dissociation equilibrium constant,stability constant(stepwise process).relationship of dissociation equilibrium constant and stability constant,calculation of equilibrium composition. Chapter 6 Precipitation-solubility equilibria (4.0 hrs) 6.1 Solubility and solubility product 6.2 Forming and dissolving of precipitates $6.3 Equilibrium between two precipitates
To know essential points of the Brønsted theory of acids and bases and basic concepts on the theory about Lewis acids and bases. To master ionization of water, standard ion-product constant of water, and calculation of pH of strong acid and strong base. To master the ionization equilibria of monoprotic weak acid and weak base, the calculation of equilibrium composition; to be familiar with equilibrium of stepwise process of polyprotic weak acid and calculation of equilibrium composition. To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base, and salt of monoprotic weak bases and strong acid, calculation of equilibrium composition, to be familiar with multi-step hydrolysis of salt of polyprotic weak acid and calculation of equilibrium composition. To master the concepts of common ion effect and buffer solution,and calculation of pH of a buffer solution. To master the basic concepts on complex, to know how to name a complex, To master complex formation reaction and its equilibrium, to know calculation of equilibrium composition, to know calculation of equilibrium composition under the condition of coexistence of equilibrium of acid and base reaction and dissociation equilibrium of complex. important and difficult points： Essential points of the Brønsted theory of acids and bases: concepts of acid, base, amphiprotic substance; conjugate acid-base pair. The essential of acid-base reaction is transfer of protons. The essential of ionization of water, ionization of acid and base, as well as that hydrolysis of salt are transfer of protons. The major content on Lewis acids and bases: the concept of Lewis acids and bases. The ligand in a complex is Lewis base. Ionization equilibrium of water: ionproduct constant of water , influence of temperature on ion-product constant of water, T = 298K, KW Q(298K)=1.0×10-14 , PH=-lg{c(H+)},POH=- lg{c(OH-)},298K时，PH+POH=14.00. Of importance is to master the ionization equilibrium in solutions of monoprotic weak acids and weak bases, ionization equilibrium constant, percent ionizaton (a), calculation of equilibrium composition and pH of a reaction, the conditions for approximate calculation and methods of calculation. To master the ionization equilibrium in solutions of salt of monoprotic weak acid and strong base, and salt of monoprotic weak bases and strong acid, the relationship between constant of ionization of water and constant of ionization of acid and base. Features of salt of polyprotic weak acids: multi-steps hydrolysis; relationship between ionization constant and hydrolysis constant; simple calculation of hydrolysis equilibrium of salt of polyprotic weak aicd and strong base (treat it as an equilibrium of hydrolysis of polyprotic base). To be familiar with concepts of ligand, coordination atom, coordination number etc about coordination compound, naming normal compounds, distinguish simple and chelating complexes, i.e., normal ligands. The dissociation equilibrium of complex (stepwise process), dissociation equilibrium constant , stability constant (stepwise process), relationship of dissociation equilibrium constant and stability constant, calculation of equilibrium composition. Chapter 6 Precipitation-solubility equilibria （4.0 hrs） § 6.1 Solubility and solubility product § 6.2 Forming and dissolving of precipitates § 6.3 Equilibrium between two precipitates
aims of teaching: To be familiar with equilibrium of dissolving and forming of a sparingly soluble electrolyte,to master standard solubility product constant,the relationship with solubility,and related calculation.To master solubility product rule,to know how to judge forming or dissolving of a precipitate based on solubility product rule. To master the effect of pH on solubility of sparingly soluble metal sulfides and metal hydroxides and related calculation;to be familiar with simple calculation of equilibrium of complexing-dissolving of precipitate.To know Equilibria between two precipitates and related calculation. important and difficult points: Definition of solubility product.Forming and dissolving of precipitates comes to an equilibrium.solubility product.Relationship between solubility and solubityroduct,andthe readcalcuo The sotproduct rue Thetino precipitationsouqba forming precipitate:p forming saturated solution;dissolving precipitate.Shift of an equilibrium between forming and dissolving of precipitate.Shift of an quilibrium can occur through either changing pH of solution,formation of complex,or transformation between two precipitate.The key point to be familiar with dissolving-forming equilibria is to understand the relationship between precipitation reaction and muti-equilibria.To deeply understand a few examples. Chapter 7 Redox Reactions and Electrochemistry (7.0 hrs) $7.1 The fundamental concepts of redox reactions $7.2 Electrochemical cells $7.3 Electrode potentials $7.4 Application of electrode potentials aims of teaching: To be familiar with basic concepts on redox reaction,and balancing redox equations using ion-electron method.To know the concepts about galvanic(voltaic) cell and electromotive force.To master the concept of electrode potential and affecting parameters,the Nernst equation and related simple calculation, application of electrode potentials.To master elemental potential diagram and its application. important and difficult points:
aims of teaching: To be familiar with equilibrium of dissolving and forming of a sparingly soluble electrolyte, to master standard solubility product constant, the relationship with solubility, and related calculation. To master solubility product rule, to know how to judge forming or dissolving of a precipitate based on solubility product rule. To master the effect of pH on solubility of sparingly soluble metal sulfides and metal hydroxides and related calculation; to be familiar with simple calculation of equilibrium of complexing-dissolving of precipitate. To know Equilibria between two precipitates and related calculation. important and difficult points: Definition of solubility product. Forming and dissolving of precipitates comes to an equilibrium. solubility product. Relationship between solubility and solubility product, and the related calculation. The solubility product rule: The reaction quotient criterion for precipitation—solubility equilibria: J > Ksp Q, forming precipitate; J = Ksp Q, forming saturated solution; J > Ksp Q, dissolving precipitate. Shift of an equilibrium between forming and dissolving of precipitate. Shift of an quilibrium can occur through either changing pH of solution, formation of complex, or transformation between two precipitate. The key point to be familiar with dissolving-forming equilibria is to understand the relationship between precipitation reaction and muti-equilibria. To deeply understand a few examples. Chapter 7 Redox Reactions and Electrochemistry（7.0 hrs） §7.1 The fundamental concepts of redox reactions §7.2 Electrochemical cells §7.3 Electrode potentials §7.4 Application of electrode potentials aims of teaching: To be familiar with basic concepts on redox reaction, and balancing redox equations using ion-electron method. To know the concepts about galvanic(voltaic) cell and electromotive force. To master the concept of electrode potential and affecting parameters, the Nernst equation and related simple calculation, application of electrode potentials. To master elemental potential diagram and its application. important and difficult points: