A CH3COOH /
NaCH3COO buffer system is to be
constructed that is also 0.044 M in
Cr3+.
What is the minimum [CH3COOH] /
[CH3COO-] that must be
maintained to keep a precipitate of chromium(III)
hydroxide from forming?
minimum |
[CH3COOH] |
= | --------- |
[CH3COO-] |
1 |
Get the minimum OH- required for precipitaiton
Ksp = [Cr+3][OH-]^3
Cr(OH)3 3×10–29
3*10^-29 = (0.044)(OH-)^3
[OH-] = ((3*10^-29)/0.044)^(1/3)
[OH-] = 8.801*10^-10
then,
[H3O+] = (10^-14)/(8.801*10^-10) = 1.136*10^-5 M
pH = -log(H3O+) = -log(1.136*10^-5) = 4.944
apply buffer equation
pH = pKa + log(NaCH3COO / CH3COOH)
4.944= 4.75 + log(NaCH3COO / CH3COOH)
NaCH3COO / CH3COOH = 10^(4.944- 4.75 ) = 1.5631
we need the inverse, so
(NaCH3COO / CH3COOH)^1 = 1.5631^-1
CH3COOH/NaCH3COO = 0.6397
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