Solubility

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Unit 7

15 Terms

1
Sparingly Soluble Salts
salts (ionic compounds) that are insoluble in water
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2
why are ionic compounds insoluble in water
the crystal lattice structure is too strong and water cannot enter, ionic bonds are too strong and water molecule cannot substitute for ionic bond
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3
molar solubility
concentration of a salt in 1L of water
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4
1:1 salts
ex: AgCl

x=√ksp
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5
1:2 salts
ex: Ag2CrO4

x=3√ksp/4
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6
1:3 salts
ex: Ag3PO4

x=4√ksp/27
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7
how to compare if ksp will form
calculate Q and compare it with ksp
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8
Q>ksp
precipitate will form
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9
Q
precipitate will not form
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10
Q=ksp
solution is just saturated
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11
Will precipitate form when 1L of 3x10^-10M Co(NO3)2 is added to 1L of 2x10^-11 K2S (ksp CoS = 5x10^-22)
  1. calculate Q and compare with ksp

  2. final volume is 2L since dilution has already occured

  3. use c1v1=c2v2 to find new [Co] and [S]

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12
if ksp is small…
many reactants are present
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13
when can we ignore +x
when ksp is very small, it means that +x is also very small and won’t change the concentration much, so 0.1 +x becomes 0.1
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14
why is there a reduction in solubility with NaCl compared to solubility in water
the Cl ions already in solution from NaCl have taken up room so not many Cl ions from AgCl can enter solution
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15
common ion effect
the reduction of solubility
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