can someone please help me with this question?

Given the aqueous solubility rules presented in this module please answer the following questions based on the information presented below: You are mixing exactly 95.0 mL of 1.5 x 10-4 M Ba(OH)2 with 35.5 mL of 2.8 x 10-5 M Fe2(SO4)3. Ksp (BaSO4) = 1.1 x 10-8 Ksp (Fe(OH)3) = 2.6 x 10-29 1. What are the possible products in this reaction mixture? 2. What are the possible IP expressions to be studied? 3. What is the concentration of Fe3+ that is being used in the appropriate IP expression? 4. Is a precipitate formed from this mixing of the two solutions, and if so, which precipitate would it be? Possible precipitate products are Ba(OH)2 and Fe2(SO4)3 Possible precipitate products are BaSO4 and Fe2(SO4)3 O [Fe3+] = 1.1 x 10-4 M OIP = [Ba2+1 [OH1-12 Possible precipitate products are Ba(OH)2 and BaSO4 Yes there is a precipitate and it is Fe2(SO4)3. Yes there is a precipitate and it is Fe(OH)3. [Fe3+] = 7.6 x 10-6M IP = [Ba2+][s0421 SO42-1 [Fe3+1 = 1.5 x 10-5 M [Fe3+] = 2.2 x 10-5M O IP = [Fe3+]2[SO42-13 Yes there is a precipitate and it is BaSO4. Possible precipitate products are BaSO4 and Fe(OH)3 OIP = [Ba2+][OH1-12 No, there will not be a precipitate formed upon the mixing of these two solutions. [Fe3+] = 2.2 x 10-4 M Yes there is a precipitate and it is Ba(OH)2. Possible precipitate products are Ba(OH)2 and Fe(OH)3 OIP = [Fe3+1(OH1-13