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Objectives Determine that all the water has been driven from hydrate by heating a sample to constant mass. Use experimental data to calculate the moles of water released by a hydrate. Infer the empirical formula of the hydrate from the formula of the anhydrous compound and experimental data. Introduction Many ionic compounds, when crystallized from aqueous solution, will take up definite amounts of water as an integral part of their crystal structures. This water of crystallization may be driven off by heating the hydrated substance to convert it to its anhydrous form. Because of the law of definite composition holds for crystalline hydrates, the number of moles of water are driven off per mole of the anhydrous compound is a simple whole number. If the formula of the anhydrous compound is known, you can use your data to determine the formula of the hydrate. Materials Balance, centigram Bunsen burner and associated utensils Crucible and cover Desiccators Iron ring Magnesium sulfate, Epsom salts, hydrated crystals Pipe-stem triangle Ring stand Sparker Spatula Tongs Procedure 1.
Approximate Word count = 591
Approximate Pages = 2.4
(250 words per page double spaced)
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