Writing the net reaction for reaction of sodium hypochlorite with hydrochloric acid and potassium bromide
I'd like to add some things to what Tanith Rosenbaun said.
First, the point of net ionic equations is not just to write out the equations in terms of ions, but to focus on only those ions that experience a change in charge or valence.  Ions which don't change in charge don't really participate in the reaction and called spectator ions.
Here's the last equation from Rosenbaum's answer:
$$\ce{2H3O+ + 2Cl- + 2Na+ + CO3^2- -&gt; 2H2O + 2Cl- + 2Na+ + CO2}$$
Notice that the sodium and chloride ions are unchanged in this reaction.  So we drop them, and just write out the ions that change:
$$\ce{2H3O+ + CO3^2- -&gt; 2H2O + CO2}$$
This is the net ionic equation: it focuses precisely on what is interesting, which in this case is the neutralization reaction.
Now let's go back to your problem:  People have been asking what you know about it.  You seem to know that you are transferring a solution of chlorine dissolved in cyclohexane.  You got that chlorine from the following reaction:
$$\ce{2HCl + NaClO -&gt; Cl2 + NaCl + H2O}$$
and the chlorine preferentially dissolves in the cyclohexane.  Now it's important to understand that the cyclohexane doesn't play any role in the second part of your experiment, it's just how you transport the chlorine.  (And it's why you need to be careful with acids around bleach: chlorine gas is poisonous!)
The key question is: what happens when you put elemental chlorine in the presence of dissolved potassium bromide?
$\ce{Cl2 + KBr -&gt; ?}$  (Note: this is not balanced yet!)
In particular, do you know what you produced when that solution turned dark red?  Hint: this is a very important property that halogens like chlorine and bromine have towards each other, which is indeed seen best via a net ionic equation.  I'll happily provide the answer if you've tried some stuff and are still stuck.