Calculate solubility of AbBr in 6.0 M NH3. Assume the highest complex formed is Ag(NH3)2 +.© BrainMass Inc. brainmass.com October 24, 2018, 5:40 pm ad1c9bdddf
This solution is provided in 204 words in an attached .doc file. It determines equilibrium concentrations in order to find the solubility of the compound.
Calculating solubility of aluminum in aluminum sulfate (AL2(SO4)3) at various pH levels?
Alum (aluminum sulfate) is used as a flocculant to floc an anionic material in a water solution at pH = 4.0 and temperature = 130 degrees F. The solubility of the alum is noted as 87 grams per 100 cc's of liquid (assuming std temp & pressure).
Assume 1 liter of solution....based on this, how would I determine the actual solubility of the aluminum ion (how much dissolved vs. not) at say a pH of 3.0 vs. 4.0 vs. 5.0.
Typical aluminum chemistry suggests that lower pH increases solubility given a fixed temperature of 130 degrees F ---- I also heretell that the optimal pH for alum chemistry is in the range of 4.5 to 5.0.
But I do not understand this and want to know how to derive the soluble vs. insoluble Al at these various pH ranges.
I am ultimately trying to drive the following:
Al(SO4)3 + 6H2O = 2Al(OH)3 + 3H2SO4
My theory being that if I have more insoluble alum sulfate, I will produce more aluminum hydroxide (assuming sufficient OH)View Full Posting Details