Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between ammonium nitrate and potassium hydroxide. It begins with balancing the molecular equation, then discusses the solubility rules and states of substances involved. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring charge conservation and summarizing the process.

What is the first step in writing a balanced net ionic equation?

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

• Identify spectator ions

According to solubility rules, what is the state of ammonium nitrate in water?

• Solid

• Gas

• Aqueous

• Liquid

Why is ammonia not split into ions in the net ionic equation?

• It is a solid

• It is a strong acid

• It is a strong base

• It is a weak base

What charge does the ammonium ion carry?

• 2+

• 1-

• 1+

• 2-

Which ion is not a spectator ion in the reaction?

• Hydroxide ion

• Ammonium ion

• Nitrate ion

• Potassium ion

What happens to the potassium ion in the net ionic equation?

• It forms a precipitate

• It is split into atoms

• It reacts with ammonia

• It is a spectator ion

What is the state of water in the net ionic equation?

• Solid

• Liquid

• Gas

• Aqueous

What is the significance of identifying spectator ions?

• They participate in the reaction

• They form new compounds

• They help balance the equation

• They do not change during the reaction

What is the net charge on both sides of the balanced net ionic equation?

• 1+

• 1-

• 0

• 2+

Why is it important to ensure charge conservation in a net ionic equation?

• To balance the atoms

• To ensure the reaction is feasible

• To maintain electrical neutrality

• To identify spectator ions