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Miniature Inorganic and Analytical Chemistry Experiments

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Miniature of Inorganic and Analytical Chemistry Experiment: Wu Maoying, Yu Qian editor of the publication time: 2013 edition Introduction "micro inorganic and analytical chemistry experiment" is the basis of many years of research and teaching experience written in the finishing. The characteristics of "Miniature Inorganic and Analytical Chemistry Experiment" are: using an instrument system with micro-sized general-purpose instruments as the main body, the average amount of reagents is reduced to about 1/10 of the conventional experiment, the experimental phenomenon is obviously credible, and the accuracy of the measurement results meets the requirements. The operating specifications are basically consistent with the constant experiments, which is very convenient for application and implementation in teaching. The experimental content and project arrangement of "Miniature Inorganic and Analytical Chemistry Experiment" are basically the same as the constant experiment, namely: introduction, laboratory common sense, experimental basic knowledge, 6 basic operation training experiments, 7 basic theory and constant determination experiments, element and There are 7 compound property experiments, 6 inorganic compound purification, extraction, and preparation experiments, 15 analytical chemistry experiments, 8 comprehensive experiments, and 7 design experiments. "Miniature Inorganic and Analytical Chemistry Experiment" can be used as a textbook or teaching reference book for inorganic and analytical chemistry experiments in chemistry, chemical engineering, materials, environment, biology, food, pharmacy, medicine, agriculture and related majors in colleges and universities.
Introduction I. Characteristics of the experimental system of this textbook and its application in teaching
1. Features
2. Teaching application effect 2. Learning requirements of inorganic and analytical chemistry experiments
1. Clear experimental purpose
2. Master the correct learning method Attachment: Example of an experimental report format Laboratory common sense I. Student experiment code Attachment: Duty of duty on duty 2. Safety rules and accident handling 3. Specification of chemical reagents 4. Analysis of laboratory water and its experimental basis Knowledge 1. Introduction to commonly used instruments 2. Basic operation techniques
1. Glass instrument washing
2. The use of chemical reagents
3.Heating method
4. Glass processing operations
5. Gas generation, purification, drying and collection
6. Evaporation and concentration and recrystallization
7. Separation of solution and precipitate
8. Pipette, volumetric flask and burette
9. Test the properties of solution and gas with test paper
10. Use of test tubes 3. Commonly used precision instruments and their use
1. Laboratory weighing instruments
2. Type 25 acidity meter
3. pHX? 3C type acidity meter
4. DDS? 11A conductivity meter
5. 721 spectrophotometer
6. Abbe refractometer
7. Moving trough type (Futing type) mercury barometer 4. Error and data processing
Measurement error
2. Significant figures
3. Data Representation and Processing in Chemical Experiments Experimental Contents Part I Basic Operation Training Experiments Experiment 1 Analytical Balance Use and Weighing Practice Experiment 2 Determination of Molar Gas Constant Experiment 3 Purification Experiment of Sodium Chloride 4 Preparation of Ammonium Ferrous Sulfate Experiment 5 Washing and calibration experiment of volumetric glass instrument 6 Preparation of solution Part 2 Basic theory and constant measurement experiment experiment 7 Determination of chemical reaction rate, order and activation energy experiment 8 Single and multi-phase ion equilibrium experiment 9 Redox reaction experiment 10 Measurement experiment of ionization constant of acetic acid 11 Measurement of solubility constant of barium sulfate by conductivity method 12 Determination of [Ti (H2O) 6] 3+, [Cu (H2O) 6] 2+ and [Cu (NH3) 6 Experiment of cleavage energy of] 2+ 13 Determination of composition and stability constant of iron (III) sulfosalicylate complex Part III Properties of elements and their compounds Experimental experiment 14 Properties of important compounds in the s region 15 Important non-parts in the p region Experiments on the properties of metal compounds 16 Experiments on the properties of important metal compounds in the p region 17 Experiments on the properties of important compounds in the d region (1)
Experiment 18: Properties of important compounds in d region (2)
Experiment 19 Properties of important compounds in the ds region Experiment 20 Coordination compounds Part IV Purification, extraction and preparation experiments Brief description of inorganic synthesis methods Experiment 21 Preparation, purification and solubility determination of potassium nitrate Experiment 22 Purification experiment of copper sulfate 23 From laver Iodine extraction experiment 24 Preparation experiment of iron oxide yellow and iron red experiment 25 Preparation of magnesium sulfate heptahydrate from "salt mud" Experiment 26 Preparation of sodium bicarbonate by ion exchange method Part 5 Analytical chemistry experiment experiment 27 Formulation of acid-base standard solution concentration And calibration experiment 28 Determination of total alkalinity in industrial soda ash (acid-base titration method)
Experiment 29 Determination of fatty acids and esters in glycerol (acid-base titration method)
Experiment 30 Preparation and calibration of EDTA standard solution 31 Determination of Ca and Mg content in limestone or dolomite (coordinate titration method)
Experiment 32 Determination of water hardness (coordinate titration method)
Experiment 33 Preparation and calibration experiment of KMnO4 standard solution 34 Determination of chemical oxygen consumption in water samples (potassium permanganate method)
Experiment 35 Determination of hydrogen peroxide content (potassium permanganate method)
Experiment 36 Preparation and calibration of sodium thiosulfate and iodine standard solution 37 Determination of copper content in copper sulfate (indirect iodometric method)
Experiment 38 Determination of Vitamin C Content (Direct Iodometric Method)
Experiment 39 Determination of iron content in iron ore (potassium dichromate method)
Experiment 40 Determination of chlorine content in soluble chlorides (silver method)
Experiment 41 Spectrophotometric determination of iron content by o-phenanthroline Part Six Comprehensive experimental experiment 42 Preparation, content analysis and application experiment of sodium thiosulfate 43 Synthesis and properties experiment of potassium tris (oxalate) iron (III) ate 44 K3 [Fe (CN) 6] room temperature solid-phase reaction experiment with KI 45 Synthesis of 4A zeolite and determination of cation exchange performance 46 Synthesis of sodium percarbonate and determination of active oxygen content 47 Preparation of polyaluminum chloride and performance of flocculating water purification Experimental experiment 48 Synthesis of low-hydrate zinc borate and experimental experiment of flame retardancy 49 Determination of aluminum and magnesium content in Weishuping tablets (coordination titration method)
Section 7 Designed Experiments 50 Preparation of Ammonium Chloride 51 Preparation of Basic Copper Carbonate 52 Preparation of Nanometer Zinc Oxide and Determination of UV and Visible Light Absorption Characteristics Experiment 53 Preparation of Ferric Trichloride Reagent from Waste Iron Chips Experiment 54 Recycling experiment of acidic etching waste liquid for making circuit boards 55 Experiment of making ammonium chloride, manganese dioxide and zinc sulfate from waste dry batteries 56 Preliminary treatment of waste liquid of inorganic and analytical chemical experiment Appendix Appendix I Identification method of common ions
1. Identification methods of common cations
2. Identification methods of common anions Appendix II Common physical and chemical data tables
1. Saturated vapor pressure of water at different temperatures
2. Solubility of metal salts of inorganic compounds and organic acids in water at different temperatures
3. Common acid and alkali concentrations in the laboratory
4. Dissociation constants of some acids and bases
5. Solubility product of poorly soluble compounds
6. Standard electrode potential (298.15K)
7. Cumulative generation constant of metal complexes (ionic strength is 0, temperature is 293 ~ 298K)
Appendix III Common Indicators
Acid-base indicator
2. Mixed acid-base indicator
3. Redox indicator
4. Coordination indicator
5. Adsorption indicator
6. Fluorescent indicator Appendix IV. Preparation of commonly used buffer solutions Appendix 5. Drying conditions of commonly used reference materials Appendix VI. Preparation of special reagents References

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