CH2BP_4P1P Analytical Chemistry

Faculty of Education
Spring 2011
Extent and Intensity
2/0/0. 4 credit(s). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Luděk Jančář, CSc. (lecturer)
Guaranteed by
doc. RNDr. Luděk Jančář, CSc.
Department of Physics, Chemistry and Vocational Education – Faculty of Education
Contact Person: Helena Pelcová
Timetable
Mon 9:45–11:25 učebna 7
Prerequisites
CH2BP_3P1P Inorganic chemistry 2
Knowledge of general, inorganic and organic chemistry.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
Course objectives
Main objectives can be summarised as follows:
to learn bases of the qualitative and quantitative analytical chemistry, instrumental analytical methods, analytical calculations and methods of processing and analysis of chemical data and results.
Syllabus
  • 1. Subject of analytical chemistry. Qualitative and quantitative analysis. Chemical and instrumental methods.
  • 2. Theoretical foundations of analytical methods. Analytical reactions. Chemical equilibria. Acid/base reactions. Acid/base theories - Arrhenius, Brönsted, Lewis. Dissotiation constants of protolytic equilibria. pH. pH calculations in strong and weak solutions of acids a bases. pH calculations of hydrolysed salts. pH calculations of buffers. pH calcultions of ampholytes. Buffers. Complex reactions. Complex equilibria. The use of complex reactions in the analytical chemistry. Precipitate reaction. Constant of solubility. Calculations of the solubility of less soluble matters. Properties and formations of precipitations. Oxidation/reduction reactions. Oxidation/reduction equilibria.
  • 3. Qualitative chemical analysis. Proof ability of analytical reactions. Basic process in qualitative chemical analysis. Preparation of reagents solutions and purity of chemicals. Preliminary proofs. Proofs in the flame. Proofs of solubility. Qualitative inorganic analysis on the wet way. The transfer of solid sample into the solution. Usual operations with solutions. Analytical procedures of ions separations. Group ions reactions. Group cations reactions. Reactions of HCl. Reactions of H2SO4. Reactions of H2S. Reactions of (NH4)2S. Reactions of KOH. Reactions of NH3. Reaction of KI. Group anionic reactions. Reactions of Ba2+ ions. Reactions of Ag+ ions. Oxidation/reduction reactions of anions. Selective reactions of cations. Characteristics of alkalic metal ions. Reactions Li+ ions. Reactions of Na+, K+, NH4+ ions. Characteristics of alkalic earth ions. Reactions of Mg2+ ions. Reactions of Ca2+, Sr2+, Ba2+ ions. Reaction of Al3+, Sn2+ and Sn4+, Pb2+ ions. Reactions of As3+ and As5+ ions. Reactions of Sb3+ and Sb5+, Bi3+ ions. Characteristics of ions of the iron group. Reactions of Fe2+ and Fe3+, Co2+, Ni2+ ions. Reaction of Cu2+, Ag+, Zn2+ ions. Reactions of Cd2+ ions. Reactions of Hg22+ and Hg2+, Cr3+ ions. Reactions of Mn2+ ions. Selective reactions of anions. Reactions of F- ions. Reactions of Cl-, Br-, I- ions. Reactions of SO42-, SO32-, S2- ions. Reactions of S2O32- ions. Reactions of NO3-, NO2-, PO43-, CO32- ions.
  • 4. Quantitative chemical analysis. Subscription, modification and transfer of the sample into solution. Weighting of the sample. Gravimetry. Basic operations in gravimetry. Precipitation. Filtration. Drying and burning. Calculations of the content of the finding component. Volumetry. Basic terms in volumetry. General procedures in volumetry. Acid/base titrations. Solutions in acidimetry and alcalimetry. Acid/base indicators. Titrations curves and the choice of the indicator. Examples of acid/base determinations. Acid/base titrations in non-water media. Complex titrations. Chelatometry. Mercurimetry. Precipitate titrations. Argentometric titrations. Oxidation/reduction titration. Indications of oxidation/reduction titrations. Oxidimetric methods. Reductometric methods.
  • 5. Evaluation of analytical results. Errors of analytical determinations. Random errors. Gauss’s normal distribution of errors, estimates of the x and s parameters, Deanův-Dixon‘s coefficient, interval of the reliability, level of the significance. Systematic errors. Student’s test, Lord‘s test. Rough errors. Grubbs‘s Q-test.
  • 6. Instrumental analysis and dividing of the instrumental analytical methods. Optical methods. Refractometry. Interferometry. Polarimetry. Emission spectral analysis. Flame photometry. Inductively Coupled Plasma - ICP. Absorption spectral analysis. Nephelometry and turbidimetry. Photoluminiscent methods. Absorption spectrometry. Spectrophotometry. Absorption photometry. Colorimetry. Atomic absorption spectrometry.
  • 7. Separation methods. Distillation. Extraction. Ions exchange. Electrophoresis. Chromatography. Gass chromatography. Liquid chromatography. Teoretical processing of chromatographic methods.
  • 8. Electrochemic methods. Potentiometry. Types of electrodes. Referent electrodes. Electrodes for pH measurements. Ion selective electrodes. Potentiometric titrations. Electrolytic methods. Electrogravimetry.
Literature
  • JANČÁŘ, Luděk and Irena JANČÁROVÁ. Analytická chemie (Analytical Chemistry). první, 2003. MZLU Brno: MZLU Brno, 2003, 195 pp. ISBN 80-7157-647-6. info
Teaching methods
lectures, theoretical preparation
Assessment methods
exam;
written (performance 60 %) and oral exam.
Language of instruction
Czech
Further comments (probably available only in Czech)
Study Materials
The course is taught annually.
General note: Prerekvizity pro zapsání předmětu: CH2BP_3P1P (Anorganická chemie 2).
Information on the extent and intensity of the course: 0.
The course is also listed under the following terms Spring 2004, Spring 2005, Spring 2006, Spring 2007, Spring 2008, Spring 2009, Spring 2010, Spring 2012, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, Spring 2018.
  • Enrolment Statistics (Spring 2011, recent)
  • Permalink: https://is.muni.cz/course/ped/spring2011/CH2BP_4P1P