2.Generate the solubility-product expression for (a)CuBr.(d)La(IO3)3.(b)HgClI.(e)Ag3AsO4.(c)PbCl2 3.What CrO42-concentration is required to (a)initiate precipitation of Ag2CrO4 from a solution that is 4.13 x 10-3 M in Ag+? (b)lower the concentration of Ag*in a solution to 9.00 x 10-7 M? 4.Define buffer capacity. 5.What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer solution that has a pH of 3.50? 6.What volume of 0.200 M HCI must be added to 500.0 mL of 0.300 M sodium mandelate to produce a buffer solution with a pH of 3.37? 10 Effect of Electrolytes on Chemical Equilibria 1教学目标 Grasp the principle and practice of Chemical Equilibria.Familiar with the calculations of Activity Coefficients; 2.教学重难点 2.1 The calculation in Chemical Equilibria; 2.2 The Effect of Electrolytes on Chemical Equilibria 3教学内容 10A The Effect of Electrolytes on Chemical Equilibria 10B Activity Coefficients 4.教学方法 The basic theory and analysis principle are taught by teaching method and student's calculation practice. 5.教学评价 Grasp the students'mastery of basic tools in Chemical Equilibria To answer the questions: 1.Make a distinction between (a)activity and activity coefficient. (b)thermodynamic and concentration equilibrium constants. 2.Explain why the activity coefficient for dissolved ions in water is usually less than that for water itself
2. Generate the solubility-product expression for (a) CuBr. (d) La(IO3)3. (b) HgClI. (e) Ag3AsO4. (c) PbCl2. 3. What CrO4 2- concentration is required to (a) initiate precipitation of Ag2CrO4 from a solution that is 4.13 x 10-3 M in Ag+? (b) lower the concentration of Ag+ in a solution to 9.00 x 10-7 M? 4. Define buffer capacity. 5. What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer solution that has a pH of 3.50? 6. What volume of 0.200 M HCl must be added to 500.0 mL of 0.300 M sodium mandelate to produce a buffer solution with a pH of 3.37? 第 10 章 Effect of Electrolytes on Chemical Equilibria 1.教学目标 Grasp the principle and practice of Chemical Equilibria. Familiar with the calculations of Activity Coefficients; 2.教学重难点 2.1 The calculation in Chemical Equilibria; 2.2 The Effect of Electrolytes on Chemical Equilibria 3.教学内容 10A The Effect of Electrolytes on Chemical Equilibria 10B Activity Coefficients 4.教学方法 The basic theory and analysis principle are taught by teaching method and student’s calculation practice. 5.教学评价 Grasp the students’ mastery of basic tools in Chemical Equilibria To answer the questions: 1. Make a distinction between (a) activity and activity coefficient. (b) thermodynamic and concentration equilibrium constants. 2. Explain why the activity coefficient for dissolved ions in water is usually less than that for water itself
3.Calculate the solubilities of the following compounds in a 0.0333 M solution of Mg(ClO4)2 using (1)activities and(2)molar concentrations: (a)AgSCN. (b)Pbl2. (c)BaSO4. (d)Cd2Fe(CN)6. Cd2Fe(CN)6(s)2Cd2++Fe(CN)4 Ksp=3.2x10-17 11 Solving Equilibrium Problems for Complex Systems 1.教学目标 Grasp the principle and practice of Multiple-Equilibrium Problems Using a Systematic Method.Familiar with the Separation of Ions by Control of the Concentration of the Precipitating Agent; 2.教学重难点 2.1 Calculating Solubilities by the Systematic Method; 2.2 Systematic Method in Solving Multiple-Equilibrium Problems 3.教学内容 11A Solving Multiple-Equilibrium Problems Using a Systematic Method 11B Calculating Solubilities by the Systematic Method 11CSeparation of Ions by Control of the Concentration of the Precipitating Agent 4.教学方法 The basic theory and analysis principle are taught by teaching method and student's calculation practice. 5.教学评价 Grasp the students'mastery of Solving Equilibrium Problems for Complex Systems To answer the questions: 1.Why are simplifying assumptions restricted to relationships that are sums or differences? 2.Why do molar concentrations of some species appear as multiples in charge-balance equations? 3.Calculate the molar solubility of PbS in a solution in which [H30+]is held constant at(a)3.0 3 10-1 M and(b)3.0 x 10-4 M. 4.What mass of AgBr dissolves in 200 mL of 0.200 M NaCN? Ag+2CN=AgCN2”B2=1.3×10
3. Calculate the solubilities of the following compounds in a 0.0333 M solution of Mg(ClO4)2 using (1) activities and (2) molar concentrations: (a) AgSCN. (b) PbI2. (c) BaSO4. (d) Cd2Fe(CN)6. Cd2Fe(CN)6(s) ↔ 2Cd2+ + Fe(CN)6 4- Ksp = 3.2 x 10-17 第 11 章 Solving Equilibrium Problems for Complex Systems 1.教学目标 Grasp the principle and practice of Multiple-Equilibrium Problems Using a Systematic Method. Familiar with the Separation of Ions by Control of the Concentration of the Precipitating Agent; 2.教学重难点 2.1 Calculating Solubilities by the Systematic Method; 2.2 Systematic Method in Solving Multiple-Equilibrium Problems 3.教学内容 11A Solving Multiple-Equilibrium Problems Using a Systematic Method 11B Calculating Solubilities by the Systematic Method 11CSeparation of Ions by Control of the Concentration of the Precipitating Agent 4.教学方法 The basic theory and analysis principle are taught by teaching method and student’s calculation practice. 5.教学评价 Grasp the students’ mastery of Solving Equilibrium Problems for Complex Systems. To answer the questions: 1. Why are simplifying assumptions restricted to relationships that are sums or differences? 2. Why do molar concentrations of some species appear as multiples in charge-balance equations? 3. Calculate the molar solubility of PbS in a solution in which [H3O+ ] is held constant at (a) 3.0 3 10-1 M and (b) 3.0 x 10-4 M. 4. What mass of AgBr dissolves in 200 mL of 0.200 M NaCN?
5.Calculate the molar solubility of ZnCO3 in a solution buffered to a pH of 7.00. 6.Silver ion is being considered for separating I-from SCN-in a solution that is 0.040 M in KI and 0.080 M in NaSCN. (a)What Ag concentration is needed to lower the I-concentration to 1.0 x 10-6 M? (b)What is the Ag'concentration of the solution when AgSCN begins to precipitate? (c)What is the ratio of SCN-to I-when AgSCN begins to precipitate? (d)What is the ratio of SCN-to I-when the Agl concentration is 1.0 x 10-3 M? 第12章Gravimetric Methods of Analysis 1教学目标 Grasp the principle and practice of Precipitation Gravimetry.Familiar with the Applications of Gravimetric Methods; 2.教学重难点 2.1 Calculation of Results from Gravimetric Data. 3.教学内容 12A Precipitation Gravimetry 12B Calculation of Results from Gravimetric Data 12CApplications of Gravimetric Methods 4.教学方法 The basic theory and analysis principle are taught by teaching method and student's calculation practice. 5.教学评价 Grasp the students'mastery of solution concentration calculation To answer the questions: 1.What are the structural characteristics of a chelating agent? 2.What is peptization and how is it avoided? 3.Treatment of a 0.2500 g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.2912 g of AgCl.Calculate the percentage of KCl in the sample. 4.What mass of AgI can be produced from a 0.512 g sample that assays 20.1%All3? 5.A 0.2121 g sample of an organic compound was burned in a stream of oxygen,and the CO2 produced was collected in a solution of barium hydroxide.Calculate the percentage of carbon in the sample if 0.6006 g of BaCO3 was formed
5. Calculate the molar solubility of ZnCO3 in a solution buffered to a pH of 7.00. 6. Silver ion is being considered for separating Ifrom SCNin a solution that is 0.040 M in KI and 0.080 M in NaSCN. (a) What Ag+ concentration is needed to lower the I- concentration to 1.0 x 10-6 M? (b) What is the Ag+ concentration of the solution when AgSCN begins to precipitate? (c) What is the ratio of SCNto I- when AgSCN begins to precipitate? (d) What is the ratio of SCNto I- when the Ag1 concentration is 1.0 x 10-3 M? 第 12 章 Gravimetric Methods of Analysis 1.教学目标 Grasp the principle and practice of Precipitation Gravimetry. Familiar with the Applications of Gravimetric Methods; 2.教学重难点 2.1 Calculation of Results from Gravimetric Data. 3.教学内容 12A Precipitation Gravimetry 12B Calculation of Results from Gravimetric Data 12CApplications of Gravimetric Methods 4.教学方法 The basic theory and analysis principle are taught by teaching method and student’s calculation practice. 5.教学评价 Grasp the students’ mastery of solution concentration calculation To answer the questions: 1. What are the structural characteristics of a chelating agent? 2. What is peptization and how is it avoided? 3. Treatment of a 0.2500 g sample of impure potassium chloride with an excess of AgNO3 resulted in the formation of 0.2912 g of AgCl. Calculate the percentage of KCl in the sample. 4. What mass of AgI can be produced from a 0.512 g sample that assays 20.1% AlI3? 5. A 0.2121 g sample of an organic compound was burned in a stream of oxygen, and the CO2 produced was collected in a solution of barium hydroxide. Calculate the percentage of carbon in the sample if 0.6006 g of BaCO3 was formed
6.A 0.6407 g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430 g.This precipitate was then strongly heated in a stream of Cl2 gas to convert the AgI to AgCl;on completion of this treatment,the precipitate weighed 0.3181 g.Calculate the percentage of chloride and iodide in the sample. 7.A 50.0 mL portion of a solution containing 0.200 g of BaCl2-2H2O is mixed with 50.0 mL of a solution containing 0.300 g of NaIO3.Assume that the solubility of Ba(IO3)2 in water is negligibly small and calculate (a)the mass of the precipitated Ba(IO3)2. (b)the mass of the unreacted compound that remains in solution. 第13章Titrations in Analytical Chemistry 1教学目标 Grasp the basic aspect of titration;understand the titration process. 2.教学重难点 2.1 The generation of titration curves; 3教学内容 13A Some Terms Used in Volumetric Titrations 13B Standard Solutions 13CVolumetric Calculations 13DGravimetric Titrations 13E Titration Curves 4.教学方法 The basic theory and analysis principle are taught by teaching method and student's calculation practice. 5.教学评价 Grasp the students'mastery of Titrations principle and process To answer the questions: 1.Distinguish between (a)the equivalence point and the end point of a titration. (b)a primary standard and a secondary standard. 2.How many millimoles of solute are contained in (a)2.95mLof0.0789MKH2P04? (b)0.2011Lof0.0564MHgC2?
6. A 0.6407 g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430 g. This precipitate was then strongly heated in a stream of Cl2 gas to convert the AgI to AgCl; on completion of this treatment, the precipitate weighed 0.3181 g. Calculate the percentage of chloride and iodide in the sample. 7. A 50.0 mL portion of a solution containing 0.200 g of BaCl2•2H2O is mixed with 50.0 mL of a solution containing 0.300 g of NaIO3. Assume that the solubility of Ba(IO3)2 in water is negligibly small and calculate (a) the mass of the precipitated Ba(IO3)2. (b) the mass of the unreacted compound that remains in solution. 第 13 章 Titrations in Analytical Chemistry 1.教学目标 Grasp the basic aspect of titration; understand the titration process. 2.教学重难点 2.1 The generation of titration curves; 3.教学内容 13A Some Terms Used in Volumetric Titrations 13B Standard Solutions 13CVolumetric Calculations 13DGravimetric Titrations 13E Titration Curves 4.教学方法 The basic theory and analysis principle are taught by teaching method and student’s calculation practice. 5.教学评价 Grasp the students’ mastery of Titrations principle and process To answer the questions: 1. Distinguish between (a) the equivalence point and the end point of a titration. (b) a primary standard and a secondary standard. 2. How many millimoles of solute are contained in (a) 2.95 mL of 0.0789 M KH2PO4? (b) 0.2011 L of 0.0564 M HgCl2?
(c)2.56 L of a 47.5 ppm solution of Mg(NO3)2? (d)79.8mLof0.1379MNH4VO3(116.98g/mol)2 3.A 0.4126-g sample of primary-standard Na2CO3 was treated with 40.00 mL of dilute perchloric acid.The solution was boiled to remove CO2,following which the excess HCIO4 was back-titrated with 9.20 mL of dilute NaOH.In a separate experiment,it was established that 26.93 mL of the HCIO4 neutralized the NaOH in a 25.00-mL portion.Calculate the molarities of the HCIO4 and NaOH. 4.Titration of the 12 produced from 0.1142 g of primary-standard KIO3 required 27.95 mL of sodium thiosulfate.Calculate the concentration of the Na2S2O3. IO+5厂+6H+312+3H0 1+25,0→2+S,0 5.The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00 mL sample to 100.00 mL.A 20.00 mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH.After cooling,the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2S04.Calculate the amount of ethyl acetate(88.11 g/mol)in the original sample in grams. CH,COOC,H,+OH→ CH,COO°+CH,OE 6.A solution was prepared by dissolving 7.48 g of KCl.MgCl2.6H2O(277.85 g/mol)in sufficient water to give 2.000 L. Calculate (a)the molar analytical concentration of KCl.MgCl2 in this solution. (b)the molar concentration of Mg2+ (c)the molar concentration of Cl2 (d)the weight/volume percentage of KCI.MgCl2.6H2O. (e)the number of millimoles of Cl2 in 25.0 mL of this solution. (f)the concentration of K*in ppm. 14 Principles of Neutralization Titrations 1.教学目标 Grasp the basic aspect of neutralization titration;understand the titration curve for weak acids/bases. 2.教学重难点 2.1 Composition of Solutions During Acid/Base Titrations; 2.2 The generation of titration curves for weak acids/bases;
(c) 2.56 L of a 47.5 ppm solution of Mg(NO3)2? (d) 79.8 mL of 0.1379 M NH4VO3 (116.98 g/mol)? 3. A 0.4126-g sample of primary-standard Na2CO3 was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was established that 26.93 mL of the HClO4 neutralized the NaOH in a 25.00-mL portion. Calculate the molarities of the HClO4 and NaOH. 4. Titration of the I2 produced from 0.1142 g of primary-standard KIO3 required 27.95 mL of sodium thiosulfate. Calculate the concentration of the Na2S2O3. 5. The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00 mL sample to 100.00 mL. A 20.00 mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH. After cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate the amount of ethyl acetate (88.11 g/mol) in the original sample in grams. 6. A solution was prepared by dissolving 7.48 g of KCl • MgCl2 • 6H2O (277.85 g/mol) in sufficient water to give 2.000 L. Calculate (a) the molar analytical concentration of KCl • MgCl2 in this solution. (b) the molar concentration of Mg2+ . (c) the molar concentration of Cl2. (d) the weight/volume percentage of KCl •MgCl2 •6H2O. (e) the number of millimoles of Cl2 in 25.0 mL of this solution. (f ) the concentration of K+ in ppm. 第 14 章 Principles of Neutralization Titrations 1.教学目标 Grasp the basic aspect of neutralization titration; understand the titration curve for weak acids/bases. 2.教学重难点 2.1 Composition of Solutions During Acid/Base Titrations; 2.2 The generation of titration curves for weak acids/bases;