Hydrated Ionic Compounds and how they fit into the molecular formula thing.
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Transcript of Hydrated Ionic Compounds and how they fit into the molecular formula thing.
![Page 1: Hydrated Ionic Compounds and how they fit into the molecular formula thing.](https://reader035.fdocuments.us/reader035/viewer/2022072005/56649cd75503460f9499f297/html5/thumbnails/1.jpg)
Hydrated Ionic Compounds
and how they fit into the
molecular formula thing
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Many ionic compounds crystallize from aqueous solution with one or more water molecules incorporated into their crystal structure.
These are called hydrated ionic compounds, or “hydrates” to their close friends.
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Hydrates have a specific number of water molecules associated with each formula unit (fu) of the compound.
eg. copper II sulfate·x hydrate—blue
The water molecules are weakly bonded, and can be removed by
heating.CuSO4·xH2O(s) + heat CuSOCuSO44(s)(s) + xH2O(g)
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MgSO4·7H2O(s) + heat MgSO4(s) + 7H2O(g)magnesium sulfate anhydrous
heptahydrate magnesium sulfate
Note:
1. The dot in the formula of an ionic hydrate does not mean multiplication. It denotes a loose association of the water molecules.
2. eg. MgSO4—without any waters of hydration—is known as anhydrous magnesium sulfate.
3. Usually the number of waters of hydration is a whole number.
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Some Ionic Hydratesformula name
CaSO4·2H2O calcium sulfate dihydrate; gypsum
CaCl2·2H2O calcium chloride dihydrate
LiCl·4H2O lithium chloride tetrahydrate
MgSO4·7H2O magnesium sulfate heptahydrate, epsom salts
Ba(OH)2·8H2O barium hydroxide octahydrate
Na2CO3·10H2O sodium carbonate decahydrate
KAl(SO4)2·12H2O potassium aluminum sulfate dodecahydrate; alum
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sample problemLet’s say you want to determine the number
of waters of hydration in hydrated barium hydroxide, Ba(OH)2·xH2O.
How would do this? What measurements would you take?
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• mass the hydrate (be more specific . . .)
• weigh empty test tube; add hydrate; reweigh
• heat test tube over bunsen burner flame to drive off water
• re-weigh test tube with anhydrous Ba(OH)2
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here are some data . . .
6.00 g of barium hydroxide hydrate is heated over a bunsen burner flame to drive off the waters of hydration.
After heating, 3.26 g of anhydrous Ba(OH)2 remains. Determine the number of waters of hydration in hydrated barium hydroxide.
Calculate the formula of Ba(OH)2·xH2O.
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set up a ratio:
mm Ba(OH)2 : mass Ba(OH)2 obtained
mm Ba(OH)2·xH2O mass hydrate heated
171.4 g : 3.26 g
y 6.00 g
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cross-multiply to solve for y:
y = 315.5 g which is
the molar mass of the hydrate.
mass of water in hydrate =
315.5 g – 171.4 g = 144.1 g which is
mass of H2O/mol hydrate. Convert to mol H2O
144.1 g/18.02 g/mol = 8 mol H2O. And so...
Ba(OH)2·8H2O is the formula of hydrate.
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Homework
p 277 13 – 18
p 278 52, 54, 57 – 60
We’ll do a version of Inv 6-C on p 286
Section Review and Chapter Review Questions are all good. Knock yourself out . . .