1. Course name: Analytical chemistry
2. Code course: 2104264                      
3. Semester credit: 3(3,0,6)
4. Degree: Second year student
5. Course hours

– Class                45 hours

– Laboratory      0 hour

– Home study     90 hours

6. Prerequisite: (a) 2104039
7. Course Objectives

The course provides students with the following skills:

– To memorize the concepts and constant in analytical chemistry

– To compute for preparation of chemical solutions

– To define and compute the pH of acid-base solutions

– To apply the formulas to outline titration curves

– To choose the indicators for titrations exactly

– To solve exercises of volumetric analysis and gravimetric methods

– To recognize the accuracy and precision of experimental data and to show how these judgments can be sharpened by the application of statistical methods.

8. Course Description

          This course provides students with the knowledge base on analytical chemistry including the general analytical chemistry, volumetric analysis, gravimetric methods, statistical analysis of experimental results.

9. Student duty

Class attandance, assay, examine acording to the regulation No. 43/2007-QĐ-BGD&ĐT date 15/08/2007 of MOET, regulation No 235/QĐ-ĐHCN-ĐT date 30/08/2007 of IUH.

10. Course material:

Textbook:

Hoàng Minh Châu, Fundamental of Analytical Chemistry, Ha Noi, 2002

Reference:

David Harvey, Modern Analytical Chemistry, The McGraw Hill Companies Inc, 2000.

11. Grades:

– Class Participation

– Assay

– Short quizzes

– Middle term

– Final term

– Other

13. Grade Rule: Follow the credit regulation
14. Course Outline:

1. Introduction to Chemical Analysis

1.1. Introduction to Chemical Analysis

1.1.1. The role of analytical chemistry

1.1.2. Category of  analytical methods

1.2. The concepts and the based principles in electrolyte solution

1.2.1. Theory of electrolysis

1.2.2. Balancing in the weak electrolyte solution

1.2.3. Units, Concentration, Stoichiometry

1.2.4. The principle of conservation of mass with an electrolyte

1.3. Preparation of solution

1.3.1. Preparation of molarity solution (C_M)

1.3.2. Preparation of normality solution (C_N)

1.3.3. Preparation of weight % solution (C %)

1.3.4. Preparation of volume/volume % (v/v%)

2. Titrimetric Methods of Analysis

2.1. Overview of titrimetry

2.1.1. Equivalence points and end points

2.1.2. Titration curves

2.1.3. Calculation in titrimetric methods of analysis

2.2. Acid-base equilibriums and acid-base titrations

2.2.1. Acid-base equilibriums in water

2.2.1.1.  Principle

2.2.1.2. Water equilibrium-pH range

2.2.1.3. K_a and K_b correlations

2.2.1.4. pH of acid-base solutions (strong acid-baz, weak acid- baz, multi-acid- baz, buffer)

2.2.2. Acid-base titrations

2.2.2.1. Principle

2.2.2.2. Theories of indicator behavior

2.2.2.4. Titration curves

2.2.2.5. Calculation of acids or bases concentration in acid-base titrations

2.2.2.6. Titration methods (Titrating strong acids and strong bases, titrating a weak acid with a strong base)

2.2.2.7. Quantitative applications of acid-base titrations (Determination of HCl, NaOH, Na₂CO₃ and NaHCO₃,   NaOH and Na₂CO₃)

2.3. Complexon Equilibriums and Complexon Titrations

2.3.1. Complexon Equilibriums

2.3.1.1 Principle

2.3.1.2. Formation constant and dissociation constant

2.3.1.4. Effect factors to durability of complex

2.3.2. Complexon titrations

2.3.2.1. Principle

2.3.2.2. Concepts of complexon

2.3.2.3. Chemistry and properties of EDTA

2.3.2.4. Theories of metal indicator behavior

2.3.2.5. The titration techniques in  complexon titrations

2.3.2.6. Titration curves

2.3.2.7. Quantitative applications of complexon titrations (Determination of Ca²⁺, Mg²⁺ and mix, Zn²⁺, Fe³⁺, Al³⁺ and mix, water hardness)

2.4. Oxidation-reduction equilibrium and oxidation – reduction titration

2.4.1. Oxidation-reduction equilibrium

2.4.1.1. The definitions of oxidant-reductant

2.4.1.2. The Nernst equation and standard electrode potential

2.4.1.3. Effect factors to standard electrode potential.

2.4.2. Oxidation – reduction titration

2.4.2.1. Principle

2.4.2.2. Electrode potential indicator

2.4.2.3. Titration curves

2.4.2.4. Representative methods (Permanganate; bichromate; iodine/thiosulfate method)

2.4.2.5. Quantitative applications of oxidation-reduction titrations (Determination of Fe²⁺, Fe³⁺ , Na₂S₂O₃ , acid ascobic )

2.5. Precipitation equilibrium and precipitation titrations

2.5.1. Precipitation equilibrium

2.5.1.1. Precipitate formation conditions

2.5.1.1. The correlations of Solubility and the solubility product K_sp

2.5.2. Precipitation titrations

2.5.2.1. Principle

2.5.2.2. Requirements for the precipitation titration

2.5.2.3. Titration curves

2.5.2.4. Representative methods (Mohr; Volhard)

2.5.2.5. Quantitative applications of precipitation titrations

3. Gravimetric Analysis

3.1. Overview of gravimetry

3.2. Requirements of precipitate formed and precipitate weighed

3.3. Steps and gravimetric techniques

3.3.1. Precipitation technique

3.3.2. Filtering the precipitate

3.3.3. Transfer the precipitate formed to precipitate weighed

3.4. Calculation in gravimetric analysis

3.4.1. Conservation of mass coefficient  K

3.4.2. The principle of conservation of mass

3.5. Quantitative applications of gravimetric analysis ( Determination of Fe³⁺, Mg²⁺)

4. Evaluating analytical data

4.1. Errors in significance testing

4.2. Characterizing experimental errors

4.2.1. Accuracy

4.2.2. Precision

4.2.3. Error and uncertainty

4.3. The distribution of measurements and results

4.4. Statistical methods for normal distributions