Lab Session 5, Experiment 4: Law of Definite Proportions
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1 Lab Session 5, Experiment 4: Law of Definite Proportions The law of definite proportions states that when two or more elements combine to form a iven compound, they do so in fixed proportions by mass. This is the same as sayin the composition of a compound is fixed. For example, sodium chloride contains 39.3% by mass sodium and 60.7% by mass chlorine. In this experiment a sample of KClO 3 will be decomposed thermally, and the oxyen produced will be expressed as a percentae of the oriinal mass of KClO 3. Experimental results will then be compared to the theoretical percentae of oxyen in KClO 3. 4A Experiment: Decomposition of a Salt 1. Add approximately 0.1 of MnO 2 to a clean, dry crucible and weih the crucible includin the catalyst. Enter the mass on line (b) below. 2. Add KClO 3 to the crucible until it is about one-third full. Mix the KClO 3 and MnO 2 thorouhly. Weih aain and enter the mass on line (a) below. 3. Place the crucible on a wire trianle supported on a rin clamp. Adjust the rin clamp to a heiht that allows the crucible to be heated with the flame of your burner. 4. Heat the crucible slowly at first. Then reulate heatin to prevent boil-over from the crucible. The objective is to completely decompose the chlorate to the chloride and oxyen; therefore, heat for about ten minutes after apparent total decomposition. Heatin should be so viorous as to cause the bottom of the crucible to low red. Heat until all purple color is one and the contents are a uniform ray color. 5. Allow the crucible to cool. Weih the crucible and enter the mass on line (d) below. 6. Compute the followin: mass of oxyen, mass of KCl, experimental percentae of oxyen, theoretical percentae of oxyen, and percent error in the experimental percentae of oxyen, calculated as [ actual yield theoretical yield /theoretical yield] 100. (a) Mass of crucible with MnO 2 and KClO 3 (b) Mass of crucible with MnO 2 (c) Mass of KClO 3 [(a) (b)] (d) Mass of crucible and contents after heatin (e) Mass of oxyen [(a) (d)] (f) Mass of KCl [(c) (e)] () Experimental percentae of oxyen % (h) Theoretical percentae of oxyen % (i) Percent error in experimental percentae of oxyen % 7. Now assume that the compound you decomposed has the formula KClO x. Note that "x" is the ratio of es of O to es of KCl. Complete the followin table. (j) Experimental es of O (k) Experimental es of KCl (l) Calculated value of above ratio (m) Formula of compound decomposed 26
2 Hydrates Hydrates are substances formed when water combines chemically in definite proportions with a salt. The ratio of water ecules to the ions of the salt is a constant. Hydrates are not mixtures. The anhydrous (without water) form of the salt is produced when all the water of hydration is lost. Some examples of hydrates are listed below: Formula (CaSO 4 ) 2 H 2 O CaSO 4 2H 2 O CuSO 4 5H 2 O MSO 4 7H 2 O Na 2 CO 3 10H 2 O Names calcium sulfate hemihydrate "plaster of paris" calcium sulfate dihydrate "ypsum" copper (II) sulfate pentahydrate "blue vitriol" manesium sulfate heptahydrate "epsom salt" sodium carbonate decahydrate "washin soda" The in the formula indicates a kind of chemical bond that usually can be easily broken. For example, copper (II) sulfate pentahydrate can be converted to anhydrous copper (II) sulfate by heatin: CuSO 4 5H 2 O (sol) CuSO 4 (sol) + 5H 2 O (as). In CuSO 4 5H 2 O the bondin involves four water ecules coordinatively bound to the Cu 2+ ion in a square planar structure (Fiure 5.1) and one ecule of water bound to the sulfate ion by hydroen bonds (Fiure 5.2). Fiure 5.1 Fiure 5.2 Loss of hydration water to the atmosphere is called efflorescence. The property of some salts to collect moisture from the air and dissolve in it is called deliquescence. A compound is hyroscopic if absorption of water from the atmosphere occurs without dissolution of the compound. 27
3 4B Experiment: Composition of a Hydrate In the followin experiment, record all masses in the data table. 1. Weih your evaporatin dish. 2. Introduce about 5 of pulverized hydrated CuSO 4. Note the appearance and color of the solid; weih the dish and contents. 3. Place the evaporatin dish on the wire auze and heat slowly until the color disappears. Proloned heatin may result in the decomposition of the anhydride. What color chane occurred? 4. When cool, weih the dish and anhydride. 5. From the data, calculate the followin: the percentae of water in the hydrate [(mass of H 2 O) (mass of hydrate)] 100, the number of es of water [(mass of H 2 O) ar mass of H 2 O], the number of es of anhydride [mass of anhydride ar mass of anhydride], and the formula of the hydrate CuSO 4 x H 2 O where x = [(es of water) (es of anhydride)]. 6. Add water a few drops at a time to convert the anhydride back to the hydrate. Do you notice a chane in temperature? (Check with a thermometer.) 7. What evidence of a chemical chane did you observe? Formula of Copper Sulfate Hydrate Experiment Duplicate (a) Mass of crucible or dish and hydrate (b) Mass of empty crucible or dish (c) Mass of hydrate [(a) (b)] (d) Mass of crucible or dish and anhydride (e) Mass of anhydride [(d) (b)] (f) Mass of water in hydrate [(c) (e)] () Percentae of water in hydrate [(f) (c)] 100 % % (h) Moles of water [(f) ar mass of H 2 O] (i) Moles of anhydride [(e) ar mass of anhydride] (j) Moles of water per e of anhydride [(h) (i)] (k) Theoretical es of water per e of anhydride (l) % error [( (j) (k) (k)) 100] (m) Formula of hydrate (n) Equation for decomposition of your hydrate 28
4 4C Experiment: Properties of hydrates 1. Place crystals of calcium chloride, washin soda, and lithium chloride on a watch lass and expose them to the air of the laboratory. 2. Note the appearance of each sample towards the end of the lab. Which crystals deliquesce? Which crystals effloresce? Explain why one sample ained water and why one lost water. 4D Experiment 1. Introduce one spatula of each of the followin into separate test tubes: sodium chloride, potassium dichromate, aluminum sulfate, cobalt chloride, and nickel sulfate. Record color before heatin in the table below. 2. Heat each sample in turn, holdin the tube at an anle of about 30º so that any water will condense in the cool part of the tube. Record color after headin in the table below. 3. When you heated salts in this experiment, which ones lost water? 4. Can the oriinal color be restored by addition of a few drops of water to the cooled tube? List any hydrates that chaned color upon heatin, but for which the color came back when water was added. (a) Sodium Chloride (b) Potassium Dichromate (c) Aluminum Sulfate (d) Cobalt Chloride (e) Nickel Sulfate Color Before Heatin Color After Heatin 29
5 Report Form 4: Law of Definite Proportions Name Partner Section # 4A Experiment: Decomposition of a Salt (a) Mass of crucible with MnO 2 and KClO 3 (b) Mass of crucible with MnO 2 (c) Mass of KClO 3 [(a) (b)] (d) Mass crucible and contents after heatin (e) Mass of oxyen [(a) (d)] (f) Mass of KCl [(c) (e)] () Experimental percentae of oxyen % (h) Theoretical percentae of oxyen % (i) Percent error in experimental percentae of oxyen % (j) Experimental es of O (k) Experimental es of KCl (l) Calculated value of above ratio (m) Formula of compound decomposed 4B Experiment: Composition of a Hydrate What color chane occurred? Do you notice a chane in temperature? (Check with a thermometer.) What evidence of a chemical chane did you observe? Experiment Duplicate (a) Mass of crucible or dish and hydrate (b) Mass of empty crucible or dish (c) Mass of hydrate [(a) (b)] (d) Mass of crucible or dish and anhydride (e) Mass of anhydride [(d) (b)] (f) Mass of water in hydrate [(c) (e)] () Percentae of water in hydrate [(f) (c)] 100 % % (h) Moles of water [(f) ar mass of water] (i) Moles of anhydride [(e) ar mass of anhydride] (j) Moles of water per e of anhydride [(h) (i)] (k) Theoretical es of water per e of anhydride (l) % error [( (j) (k) (k)) 100] (m) Formula of hydrate (n) Equation for decomposition of your hydrate 30
6 4C Experiment: Properties of hydrates Which crystals deliquesce? Which crystals effloresce? Explain why one sample ained water and why one lost water. 4D Experiment When you heated salts in this experiment, which ones lost water? Can the oriinal color be restored by addition of a few drops of water to the cooled tube? List any hydrates that chaned color upon heatin, but for which the color came back when water was added. (a) Sodium Chloride (b) Potassium Dichromate (c) Aluminum Sulfate (d) Cobalt Chloride (e) Nickel Sulfate Color Before Heatin Color After Heatin 31
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