Your colleague recently performed an experiment that you wish to replicate. The

ID: 577240 • Letter: Y

Question

Your colleague recently performed an experiment that you wish to replicate. The experiment

was a reaction of Barium Chloride and Iron (III) Sulfate which resulted in precipitation of

Barium Sulfate out of the solution. You read through your colleague's notes and realize to your

dismay that they were poorly written and incomplete. You know that your colleague obtained

4.58g of Barium Sulfate and used 2.45g of Iron(III) Sulfate to get this much. You also know that

your colleague used Barium Chloride Dihydrate and obtained a hydrated Barium Sulfate product.

However, you cannot tell from the notes the mass of the Barium Chloride dihydrate used or the

waters of hydration of the Iron (III) sulfate used or the Barium Sulfate collected. Luckily, your

colleague mentioned the Barium Sulfate weighed 3.5g immediately after oven drying. Given this

information, what are the waters of hydration of the Iron (III) Sulfate and Barium Sulfate, and

what is the mass of the Barium Chloride Dihydrate that was used?

The question is quite simple to calculate the hydartion of waters.

First calculate the mass of water. = 4.58-3.5 g = 1.08 gm

moles of water = 1.08/18.05 = 0.060

moles of barium sulfate = 3.5/233.38 = 0.015

Mole Ratio , nBa(SO4) = 1

n (H2O) = 4

So BaSO4 contains 4 molecules of hydration. Ba(SO4).4H2O

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