- •Experiments
- •In the Laboratory
- •1. Handling the Bunsen burner
- •2. Handling chemical reagents
- •3. Handling glassware
- •4. Heating procedure
- •Seminar 1 chemical equivalent. Law of equivalents
- •Questions and problems
- •Seminar 2 rate of a chemical reaction. Chemical equilibrium
- •Questions and problems
- •Experiment 1
- •Ionic equilibrium
- •1. Dissociation of weak electrolytes
- •1. Formation and dissolution of a precipitate
- •2. Direction of a chemical reaction
- •3. Heterogenous equilibrium
- •Questions and problems
- •Experiment 3
- •Ionic product of water. Ph. Hydrolysis of salts
- •1. Determination of pH of solutions of some salts
- •Experiment 4 oxidation-reduction reactions
- •Concentrated sulfuric acid
- •Experiment 5 complex (coordinate) compounds
- •1. Formation of complex compounds
- •2. Destruction of complex compounds
- •4. Dissociation of complex compounds
- •Questions and problems
- •Experiment 6
- •(Alkaline and alkaline earth metals)
- •Biological significance of alkaline metals
- •Biological and agricultural properties of elements of
- •Iia group
- •1. Interaction of sodium with air and water
- •Experiment 7 elements of iiia and iva groups
- •Biological properties of boron and aluminum
- •1. Properties of boric acid and its salts
- •Experiment 8 elements of va and via groups
- •Biological importance of sulfur
- •1. Formation and properties of ammonia
- •2. Oxidizing properties of nitric acid
2. Oxidizing properties of nitric acid
Heat carefully a test tube with 2-3 ml of concentrated nitric acid and add a smouldered piece of coal. Observe evaluation of a brown gas of NO2. Write down and balance the reaction.
3. Redox duality of nitrites
a) Take 1 ml of sodium nitrite in a test tube, add 1 ml of potassium iodide and 1 ml of 2 N sulfuric acid. Observe evaluation of iodine.
b) Take 1 ml of sodium nitrite into a test tube, add 1 ml of 2 N sulfuric acid and 5 drops of potassium permanganate.
Write down and balance the reactions (a) and (b).
4. Reducing properties of sulfides
Take 1 ml of an aqueous solution of iodine and add some drops of potassium sulfide solution. Write down and balance the reaction.
5. Formation of sulfides
Take 5 test tubes filled with Zn, Mn(II), Cd, Sn(II) and Pb(II) salts respectively and add potassium sulfide into each test tube. Observe colors of the formed sulfides.
6. Reducing properties of sulfites
Take 1 ml of potassium dichromate into a test tube, add sulfuric acid and sodium sulfite solution. Write down and balance the reaction.
7. Oxidizing properties of sulfuric acid
Take 2 ml of concentrated sulfuric acid in the test tube (be careful!) and add some pieces of copper. Heat the test tube if necessary. Observe the evaluation of sulfur dioxide. Write down and balance the reaction.
QUESTIONS AND PROBLEMS
Describe the electronic structure of ammonia and NH4+ ion.
Using the molecular orbital method draw molecular diagrams of N2 and O2 molecules. Compare stabilities of these molecules.
Calculate pH of 0.01 M solution of NH4OH.
Calculate the solubility of Ag2SO4: (a) in pure water; (b) in presence of 0.1 M solution of sulfuric acid.
Compare solubilities of MnS and CuS in diluted hydrochloric acid.