# Write the balanced molecular equation, complete ionic equation, and net ionic equation for the...

## Question:

Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction that occurs between aqueous solutions of sodium hydroxide and potassium iodate.

## Net Ionic Equations

Net ionic equations are chemical equations that summarize the important parts of a chemical reaction that would take place given a balanced chemical reaction. The net ionic equation eliminates spectator ions so if all ions are removed, it is likely that no reaction will take place.

We are given aqueous solutions of sodium hydroxide {eq}NaOH {/eq} and potassium iodate {eq}KIO_3 {/eq}

a. Balanced Molecular Equation

To write the balanced chemical equation, we have to make a chemical equation of sodium hydroxide having a double displacement reaction with potassium iodide.

$$NaOH + KIO_3 \to NaIO_3 + KOH$$

We can see that the reactants and the products have an equal number for each element, so this equation is balanced.

b. Complete Ionic Equation

To write a complete ionic equation, we can refer to the balanced chemical equation and split each compound into its ions. potassium iodate will be split into potassium cation and iodate anion, sodium hydroxide will be split into sodium cation and hydroxide anion, sodium iodate will be split into sodium cation and iodate anion, and potassium hydroxide would be split into potassium cation and hydroxide anion.

$$Na^+ + OH^- + K^+ + IO_3^- \to Na^+ + IO_3^- + K^+ + OH^- \\$$

We can see that the reactants and the products have an equal number for each ion, so this equation is balanced.

c. To write a net ionic equation, we have to check the solubility of the products and the reactants of the balanced chemical equation. By checking the solubility rules, we could see that all participating compounds are soluble in water and would exist in ionic form. There would be no net ionic equation as all reactants and products exist in ionic form