CoCl2+NaOH
I don't understand the process of net ionic equations at all:mad:

The idea of a net ionic equation is actually not complicated. In (usually) aqueous solutions, compounds separate into ions. Some of the ions participate in a reaction, while other ions just sit around. The latter are called "spectator ions". They remain in solution and don't really do much.

In your case, the following occurs:

CoCl_2\, +\, NaOH\, =\, Co^{+2}\, +\, 2\,Cl^- + Na^+, + \,OH^-

After that, you have to have some idea of what might occur. Sodium (Na+) and Chloride (Cl-) are typical ions that oftendo little. In this case, they certainly don't do anything. The only thing that can really occur is that Cobalt(II) and Hydroxide (OH-) could react to form Co(OH)2

Co^{+2}\,+\,2\,OH^- = Co(OH)_2

The driving force would be the formation of somewhat insoluble Cobalt(II)Hydroxide. That, therefore, is the net ionic equation for this reaction -- the chemical equation that only contains the ions of interest in the reaction.