What is the correct and balanced chemical equation for complete dissociation of Fe2(SO4)3 in water? {Hint: look up the polyatomic ion "sulfate ion" in chapter 5 of your book or online, before answering this question}. II) If a solution has molar concentration of 2.00 mol/L of  Fe2(SO4)3, then what is its total molar ion concentration?

I) The correct and balanced chemical equation for the complete dissociation of Fe2(SO4)3 in water is:

Fe2(SO4)3 (s) → 2 Fe3+ (aq) + 3 SO4^2- (aq)

This equation shows that one molecule of Fe2(SO4)3 dissociates into two Fe3+ ions and three SO4^2- ions in water.

II) The total molar ion concentration can be calculated by multiplying the molar concentration of Fe2(SO4)3 by the total number of ions produced per formula unit.

In this case, one formula unit of Fe2(SO4)3 produces 2 Fe3+ ions and 3 SO4^2- ions, for a total of 5 ions.

Therefore, if the molar concentration of Fe2(SO4)3 is 2.00 mol/L, the total molar ion concentration would be 2.00 mol/L * 5 = 10.00 mol/L.