Write an equation for the reaction between the Bronsted-Lowry acid HOCl(aq) reacting with base CO32-(aq)

I am having difficulty with this question. Here is what i have so far but I know i went wrong somewhere.

HOCl (aq) + CO32-(aq) --> HCO3-(aq) + OCl(aq)

Any help would be great!

You have the reaction.

To write the correct equation for the reaction between the Bronsted-Lowry acid HOCl(aq) and the base CO32-(aq), we need to make sure that both the acid and the base component react completely to form new products.

The chemical formula for HOCl is correct. However, the chemical formula for CO32- is incorrect.

The correct chemical formula for CO32- is:
CO32-(aq) + 2H2O(l) <=> HCO3-(aq) + OH-(aq)

Now, let's write the complete balanced equation for the reaction between HOCl(aq) and CO32-(aq):

HOCl(aq) + CO32-(aq) + 2H2O(l) <=> HCO3-(aq) + OH-(aq) + OCl-(aq)

In this balanced equation, the HOCl donates a proton (H+) to CO32-, forming HCO3-, while the remaining part of HOCl (OCl-) remains as an anion.

Remember that in Bronsted-Lowry acid-base reactions, acids donate protons (H+ ions) while bases accept protons.