A chemist has a sample of hydrated FeCl_3 and it weighs 5.0 grams. He heats it strongly to drive...
Question:
A chemist has a sample of hydrated {eq}FeCl_3{/eq} and it weighs {eq}5.0{/eq} grams. He heats it strongly to drive off water of hydration, and after heating, he found that the anhydrous compound has a mass of {eq}3.0{/eq} grams.
Find the formula of the hydrate.
Water Of Crystallization
Some molecules, when forming crystals, absorb water from the surroundings and lock them into the crystal structure. However, this is not a chemical reaction: when heated strongly, this water of crystallization can be removed from the compound. The dry form is called 'anhydrous', while the one with water present is termed 'hydrated'.
Answer and Explanation: 1
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View this answerWe can quantify the number of grams of water driven off by subtracting the mass of the anhydrous (water-less) form from the hydrated compound:
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Hydrates: Determining the Chemical Formula From Empirical Data
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Chapter 9 / Lesson 8
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Learn the anhydrate definition and what a hydrated compound is. Understand what an anhydrate is, the hydrate formula, and how to find the formula of the hydrate.
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