Determine whether the solution is basic, acidic, or neutral. Write net ionic equations to show how it behaves in aqueous solutions.

1) Fe2(SO4)3

I know it is acidic
Do I do hydrolysis equations for the net ionic or do I do redox reactions?

I'm assuming it means to write the net ionic equation, so just Fe2(SO4)3 breaking down into its polyatomic ions, which would in this case be Fe2(SO4)3(aq) -> 2Fe3(+)(aq) + SO4(2-)(aq)

But how does that show how this behaves in aqueous solution? I guess I thought it would be hydrolysis equations because that determines that the solution is basic/acidic/or neutral?

To determine whether the solution of Fe2(SO4)3 is basic, acidic, or neutral, we need to consider the behavior of the compound in aqueous solutions.

Fe2(SO4)3 is an ionic compound that dissociates in water to form Fe3+ ions and SO4^2- ions. Since Fe3+ is a transition metal cation, it can undergo hydrolysis in water.

When Fe3+ ions hydrolyze, they react with water molecules to form hydronium ions (H3O+):

Fe3+ + 3H2O -> Fe(OH)3 + 3H3O+

The formation of hydronium ions indicates that the solution is acidic. So, Fe2(SO4)3 is an acidic solution.

Now let's consider the net ionic equation for the hydrolysis reaction:

Fe3+ + 3H2O -> Fe(OH)3 + 3H3O+

The net ionic equation only includes the species that are directly involved in the reaction. In this case, Fe3+ and H2O are the reactants, and Fe(OH)3 and H3O+ ions are the products. Therefore, the net ionic equation is:

Fe3+ + 3H2O -> Fe(OH)3 + 3H3O+

You would not perform redox reactions in this case because there is no change in oxidation states between Fe3+ and Fe(OH)3.