2a) i) Define molar heat of neutralization. ii) Write an ionic equation for the reaction between KOH and HCl.

2a) i) Define molar heat of neutralization.
The molar heat of neutralization is the heat energy change that occurs when one mole of water is formed from the reaction between an acid and a base under standard conditions.

2a) ii) Write an ionic equation for the reaction.
The reaction is between potassium hydroxide ($\text{KOH}$) and hydrochloric acid ($\text{HCl}$).
The full balanced chemical equation is:

$$\text{KOH(aq)} + \text{HCl(aq)} \to \text{KCl(aq)} + \text{H}_2\text{O(l)}$$

The complete ionic equation is:

$$\text{K}^+\text{(aq)} + \text{OH}^-\text{(aq)} + \text{H}^+\text{(aq)} + \text{Cl}^-\text{(aq)} \to \text{K}^+\text{(aq)} + \text{Cl}^-\text{(aq)} + \text{H}_2\text{O(l)}$$

Cancelling out the spectator ions ($\text{K}^+$ and $\text{Cl}^-$), the net ionic equation is:

$$$$