1. Consider this solubility equilibrium:Ag2CO3⇌2Ag+1(aq)+ CO3-2(aq)Ksp = 8.52 x 10 ̄17 a.Calculate the solubility of Ag2CO3in pure water. b.Calculate the solubility of Ag2CO3in a solution containing 7.63x 10 ̄3M K2CO3. 2. What is the solubility of BaSO4in 3.45x10-4M Na2SO4? (Ksp for BaSO4=1.08x10-10) 3.  Will a precipitate form if 30.0mL of a 7.5x10-5M KCl is added to 15mL of a 1.5x10-8M AgNO3? (Ksp AgCl = 1.8x10-10 4. 56.9 ml of 1.77 x 10–5M Al2(SO4)3is going to be mixed with 145 ml of 7.10 x 10–4M BaCl2. What precipitate might form? Determine if there is a precipitate or not.

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