what are the net ionic equations for ClO3^-; Zn^2+ undergo hydrolysis?

To determine the net ionic equation for the hydrolysis of ClO3^- (chlorate ion) and Zn^2+ (zinc ion), we need to understand how each species reacts with water.

First, let's break down the reaction of ClO3^- with water (H2O):

ClO3^- + H2O -> ?

Chlorate (ClO3^-) is a strong base that readily accepts a proton (H+) from water. This results in the formation of the hydroxide ion (OH^-) and the hypochlorite ion (ClO^-):

ClO3^- + H2O -> OH^- + ClO^-

Now, let's focus on the hydrolysis of Zn^2+:

Zn^2+ + H2O -> ?

Zinc ions (Zn^2+) have a tendency to hydrolyze and form zinc hydroxide (Zn(OH)2):

Zn^2+ + 2H2O -> Zn(OH)2 + 2H+

The net ionic equation is obtained by eliminating spectator ions, which are ions that do not participate in the reaction and appear on both sides of the equation. The spectator ion in this case is OH^-, as it appears on both sides of the equation:

ClO3^- + H2O -> OH^- + ClO^-
Zn^2+ + 2H2O -> Zn(OH)2 + 2H+

Therefore, the net ionic equation for the hydrolysis of ClO3^- and Zn^2+ is:

2OH^- + Zn^2+ -> Zn(OH)2

This equation represents the essential chemical transformation that occurs during the hydrolysis reaction.