How to Balance the Net Ionic Equation for AgNO₃ + K₂CrO₄

Both AgNO₃ and K₂CrO₄ are considered strong electrolytes and will dissociate completely. This means that we will split them apart in the net ionic equation.

AgNO₃ + K₂CrO₄ is a double displacement reaction. The Ag in AgNO₃ and the K in K₂CrO₄ switch places in the reaction.

Video: AgNO₃ + K₂CrO₄ (Net Ionic Equation)

To balance net ionic equations we follow these general rules:

1. Write the balanced molecular equation.
2. Write the state (s, l, g, aq) for each substance.
3. Split strong electrolytes into ions (the complete ionic equation).
4. Cross out the spectator ions on both sides of complete ionic equation.
5. Write the remaining substances as the net ionic equation.

Note: charges in a net ionic equation are conserved. This means that the overall charge (called the net charge) on the reactants side (left) of the equation must equal to the net charge on the products side (right).

Video: How to Balance Net Ionic Equations

More Worked examples of Net Ionic Equations

• AgNO₃ + K₂CrO₄ (example of a double displacement net ionic)
• Na₂CO₃ + CuSO₄ (another double displacement reaction)
• HNO₃ + NaOH (Strong Base and Strong Acid)
• NaOH + CH₃COOH (Strong Base and Weak Acid)
• Na₂CO₃ + AgNO₃