Imagine you are working in a lab, and you want to prepare a solution of cobalt(II) chloride. You know that the chemical is purchased in the solid form as a hydrate. You find the reagent bottle containing a vibrant purple solid; however, the chemical formula and molecular weight are obscured such that you can't read how many waters are associated with the ionic solid. You don't want to be wasteful, so you decide to determine the number of waters by heating the solid and taking the mass difference (a la the hydrate lab!). You carefully weigh out exactly 1.0096 g of the unknown hydrate. You gently heat the compound over a low flame until the mass stops changing and the deep purple color fades. The mass of the remaining compound is 0.6492 g. Determine the chemical formula of the original compound.
Imagine you are working in a lab, and you want to prepare a solution of cobalt(II) chloride. You know that the chemical is purchased in the solid form as a hydrate. You find the reagent bottle containing a vibrant purple solid; however, the chemical formula and molecular weight are obscured such that you can't read how many waters are associated with the ionic solid. You don't want to be wasteful, so you decide to determine the number of waters by heating the solid and taking the mass difference (a la the hydrate lab!). You carefully weigh out exactly 1.0096 g of the unknown hydrate. You gently heat the compound over a low flame until the mass stops changing and the deep purple color fades. The mass of the remaining compound is 0.6492 g. Determine the chemical formula of the original compound.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter1: The Nature Of Chemistry
Section: Chapter Questions
Problem 127QRT
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Imagine you are working in a lab, and you want to prepare a solution of cobalt(II) chloride. You know that the chemical is purchased in the solid form as a hydrate. You find the reagent bottle containing a vibrant purple solid; however, the chemical formula and molecular weight are obscured such that you can't read how many waters are associated with the ionic solid. You don't want to be wasteful, so you decide to determine the number of waters by heating the solid and taking the mass difference (a la the hydrate lab!). You carefully weigh out exactly 1.0096 g of the unknown hydrate. You gently heat the compound over a low flame until the mass stops changing and the deep purple color fades. The mass of the remaining compound is 0.6492 g. Determine the chemical formula of the original compound.
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