For the following chemical reaction

HCN(aq)+KOH(aq)--->H2O(l)+KCN(aq)
Write the net ionic equation, including the phases.

1. Balance the equation. That's done.

2. Separate into ions with the following rules.
a. If weak acid or weak base or weak electrolyte (such as H2O), keep as molecule.
b. If solid, keep as molecule.
c. If gas, keep as molecule
d. All others show as ions.
This step gives the complete ionic equation.

3. Cancel ions that appear on both sides of the equation. The result is the NET ionic equation.

4. What is left is the net ionic equation.

To write the net ionic equation, you need to first write the balanced molecular equation for the given chemical reaction. Let's break down the steps to get to the net ionic equation:

Step 1: Write the balanced molecular equation:
HCN(aq) + KOH(aq) → H2O(l) + KCN(aq)

This equation represents the reactants (HCN and KOH) combining to form the products (H2O and KCN). The state of each compound is indicated in parentheses, where "aq" represents aqueous (dissolved in water) and "l" represents liquid.

Step 2: Split the aqueous compounds into their respective ions (if applicable):
HCN(aq) → H+(aq) + CN-(aq)
KOH(aq) → K+(aq) + OH-(aq)

In this case, HCN dissociates into H+ and CN- ions, while KOH dissociates into K+ and OH- ions.

Step 3: Determine which ions are spectator ions:
In a net ionic equation, spectator ions are the ions that do not take part in the chemical reaction and remain unchanged throughout the reaction. These ions can be omitted, reducing the equation to only show the ions involved in the reaction.

In our case, K+ is a spectator ion because it does not take part in any chemical changes. Therefore, it can be omitted from the net ionic equation.

Step 4: Write the net ionic equation:
The net ionic equation includes only the ions that are involved in the reaction. In this case, the net ionic equation would be:

H+(aq) + CN-(aq) + OH-(aq) → H2O(l) + CN-(aq)

Please note that the CN- ion appears on both sides of the equation. This is because it acts as both a reactant and a product.