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18 Dec 2019

A solution has [Al3+]= 8.0×10−2 M and [CH3COOH]= 1.10 M . What is the maximum quantity of NaCH3COO that can be added to 200.0 mL of this solution before precipitation of Al(OH)3(s) begins?

For the equilibrium
Al(OH)3(s)⇌Al3++3OH−(aq)
Ksp=1.3×10−33

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Patrina Schowalter
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Related questions

For the equilibrium Al(OH)3(s) <---> Al+3 (aq)+3OH-(aq) Ksp=1.3x10-33

A solution has [Al+3] = 0.050M and [HC2H3O2] = 1.00M. What is the maximum quantity (in grams) of NaC2H3O2 that can be added to 200.0mL of this solution before precipitation begins?

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1)Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0220 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, Ksp, can be found here.(1.20x10^-5)
What percentage of the Ca2 (aq) can be precipitated from the Ag (aq) by selective precipitation?

2) Suppose a solution contains 0.24 M Pb2 and 0.49 M Al3 . Calculate the pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found here.

Suppose a solution contains 0.25 M Pb2 and 0.46 M Al3 . Calculate the pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found here.

Ksp Al(OH)3 = 4.6x10^-33

Pb(OH)2 = 1.43x10-20

minimum < pH < maximum

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