Salts are compounds composed of a metal ion plus a non-metal (or polyatomic) ion, e.g., sodium chloride (NaCl), and sodium phosphate (Na 3 PO 4 ).
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1 Experiment 4 Water of Hydration Objective - Determine the percent of water in a hydrate. Introduction Salts are compounds composed of a metal ion plus a non-metal (or polyatomic) ion, e.g., sodium chloride (NaCl), and sodium phosphate (Na 3 PO 4 ). Hydrated salts (or Hydrates) are salts, which have a definite amount of water chemically combined. Some common hydrates are: CuSO 4 5H 2 O Copper (II) sulphate pentahydrate MgSO 4 7H 2 O Magnesium sulphate heptahydrate CoCl 2 6H 2 O Cobalt (II) chloride hexahydrate SnCl 2 2H 2 O Tin (II) chloride dihydrate The dot indicates an attractive force between the polar water molecules and the positively charged metal ion. On heating, the attractive forces are overcome and the water molecules are released leaving behind the anhydrous salt. The water released on heating is called the water of hydration. Since heat is absorbed during this process, the reaction is "endothermic". (In an "exothermic" reaction heat is liberated.)
2 CuSO 4 5H 2 O decomposes at temperatures greater than 560 o C. Therefore, avoid letting the flame of the Bunsen burner rest on one spot of the crucible. Heat gently by holding the Bunsen burner in a sweeping motion. When CuSO 4 5H 2 O decomposes a black solid, CuS, is formed. Apparatus: 1. Porcelain crucible with lid * 2. Clay triangle * 3. Ring clamp * 4. Crucible tongs 5. Spatula ml beaker 7. Bunsen burner * 8. Goggles 9. Desicooler * Solids: Sample of hydrated salt (CuSO 4 5H 2 O) * View photos on course website
3 Procedure: Part A - Removing Water from a Hydrated Salt * 1. Obtain a clean crucible and lid from your instructor. Inspect the crucible for cracks. 2. Use an analytical balance and determine the mass of the empty crucible. Record the mass of the empty crucible to four decimal places on the data sheet. Record the mass of the empty crucible to four decimal places on the data sheet. 3. Use an analytical balance and weigh approximately 4.0 +/- 0.1 grams of hydrate into the crucible. Record the mass of the crucible and the hydrate to four decimal places on the data sheet. 4. Place the crucible on the clay triangle and heat gently by holding the Bunsen burner in a sweeping motion for about 12 minutes. 5. Allow to cool to room temperature inside the desicooler and weigh the crucible and the content. Record the mass of the crucible and the content (after 1st heating) to four decimal places on the data sheet. 6. After weighing, place the crucible back on the clay triangle and reheat content for about 5 minutes. Allow to cool and reweigh. Record the mass of the crucible and the content (after re-heating) to four decimal places on the data sheet. If you have done a good job in heating, the mass of the crucible and residue after the 1st heating and the 2nd heating should not differ by more than 0.01 gram. * View photos on course website
4 Part B - Add water to an Anhydrous Salt 1. Add about 30 ml of distilled water to a 50 ml beaker. Record the temperature of the water. 2. Using a spatula, transfer a scoop of CuSO 4 into the water and stir gently. Record the highest temperature reached. NOTE: Anhydrous CuSO 4 is a white compound with a bluish tint.* * View photos on course website
5 Datasheet: Part A - Removing Water from a Hydrated Salt 1. Mass of empty crucible 2. Mass of crucible and hydrated salt (CuSO 4 5H 2 O) 3. Mass of crucible and content (after 1st heating) 4. Mass of crucible and content (after re-heating) 5. Mass of used 6. Mass of anhydrous CuSO 4, which remains after heating 7. Mass of water released Calculation of % water in CuSO 4 5H 2 O (experimental): Calculation of % water (theoretical):
6 Datasheet: Part B - Add water to an Anhydrous Salt 1. Appearance of CuSO 4 5H 2 O (s) 2. Appearance of CuSO 4 (s) 3. Initial temperature of water 4. Maximum temperature reached after the addition of CuSO 4 (s)
7 Postlab Questions: 1. Briefly explain observations of the temperature changed observed in Part B of the experiment. 2. Write the chemical and word equations for any reaction(s), which occur. 3. Discuss the two most significant sources of error which are in the design of this experiment. Do not include human error as the sources of error. 4. Write the chemical and word equation for the reaction which occurs when the hydrated salt is heated. Is this an endothermic or exothermic reaction? Explain. 5. Calculate the percent water in sodium dichromate dihydrate (NaCr 2 O 7 2H 2 O).
Copper (II) sulfate pentahydrate Calcium sulfate dihydrate Magnesium sulfate heptahydrate Zinc sulfate heptahydrate
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