Net Ionic Equations and Solubility

The video tutorial explains how to write a balanced net ionic equation for the reaction between silver nitrate and ammonium iodide. It begins with balancing the molecular equation, followed by determining the solubility and states of the compounds involved. The formation of a precipitate, silver iodide, is discussed, and the complete ionic equation is derived by splitting strong electrolytes into ions. Spectator ions are identified and removed to obtain the net ionic equation. The tutorial concludes by ensuring the charge balance and atom count are correct, resulting in a neutral compound.

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

• Write the complete ionic equation

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

Which of the following is generally soluble according to solubility rules?

• Silver compounds

• Nitrates

• Iodides

• Chlorides

What is the role of solubility rules in writing net ionic equations?

• To identify spectator ions

• To determine the charge of ions

• To predict the formation of precipitates

• To balance the molecular equation

Why is silver iodide considered insoluble in this reaction?

• It dissolves in water

• It forms a precipitate

• It is a strong electrolyte

• It reacts with ammonium

Which compound forms a solid precipitate in this reaction?

• Ammonium iodide

• Silver nitrate

• Silver iodide

• Ammonium nitrate

What is the charge of the silver ion in the complete ionic equation?

• 1-

• 2+

• 0

• 1+

Which ions are considered spectator ions in this reaction?

• Silver and iodide ions

• Ammonium and nitrate ions

• Silver and nitrate ions

• Ammonium and iodide ions

What is the net charge of the balanced net ionic equation?

• 2+

• 1+

• 1-

• 0

What happens to the spectator ions in the net ionic equation?

• They change their charge

• They are removed from the equation

• They are included in the final equation

• They form a precipitate

How do you ensure the net ionic equation is balanced?

• By changing the coefficients of products

• By removing all ions

• By ensuring equal number of atoms and charges on both sides

• By adding more reactants