The “alum” used in cooking is potassium aluminum sulfate hydrate, KAl(SO4)2 ∙ x H2O. To find the value of x, you can heat a sample of the compound to drive off all of the water and leave only KAl(SO4)2. Assume you heat 4.74 g of the hydrated compound and that the sample loses 2.16 g of water. What is the value of x?
The “alum” used in cooking is potassium aluminum sulfate hydrate, KAl(SO4)2 ∙ x H2O. To find the value of x, you can heat a sample of the compound to drive off all of the water and leave only KAl(SO4)2. Assume you heat 4.74 g of the hydrated compound and that the sample loses 2.16 g of water. What is the value of x?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter3: Mass Relations In Chemistry; Stoichiometry
Section: Chapter Questions
Problem 93QAP: A sample of cocaine, C17H21O4N, is diluted with sugar, C12H22O11. When a 1.00-mg sample of this...
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4. The “alum” used in cooking is potassium aluminum sulfate hydrate, KAl(SO4)2 ∙ x H2O. To find the value of x, you can heat a sample of the compound to drive off all of the water and leave only KAl(SO4)2.
Assume you heat 4.74 g of the hydrated compound and that the sample loses 2.16 g of water. What is the value of x?
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