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Chemistry | 12th Edition | ISBN: 9780078021510 | Authors: Raymond Chang; Kenneth Goldsby
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Answer: A 5.012-g sample of an iron chloride hydrate was

Chapter 4, Problem 4.128

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QUESTION:

A 5.012-g sample of an iron chloride hydrate was dried in an oven. The mass of the anhydrous compound was 3.195 g. The compound was then dissolved in water and reacted with an excess of AgNO3. The AgCl precipitate formed weighed 7.225 g. What is the formula of the original compound?

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QUESTION:

A 5.012-g sample of an iron chloride hydrate was dried in an oven. The mass of the anhydrous compound was 3.195 g. The compound was then dissolved in water and reacted with an excess of AgNO3. The AgCl precipitate formed weighed 7.225 g. What is the formula of the original compound?

ANSWER:

Step 1 of 5

Here we have to determine the molecular formula of the ron chloride hydrate. We can use the results of several experiments to determine the number of hydrated and the number of chlorides in the formula

Let’s determine the number of moles of hydrates by using the differences in mass between the iron chloride hydrate and the anhydrous iron chloride.

From the given,

Mass of Iron chloride = 5.012g

Mass of anhydrous compound = 3.195g

                       

                                                       

 

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