Net Ionic Equations and Solubility

This video tutorial explains how to balance the net ionic equation for aluminum nitrate and ammonium carbonate. It begins with balancing the molecular equation and then moves on to determining the states of each substance using solubility rules. The tutorial explains how to split strong electrolytes into ions to form the complete ionic equation and identifies spectator ions to derive the net ionic equation. The video concludes with a balanced net ionic equation, ensuring both atoms and charges are balanced.

What is the first step in balancing a net ionic equation?

• Determine the solubility of compounds

• Identify spectator ions

• Balance the molecular equation

• Write the net ionic equation

According to solubility rules, which of the following is generally soluble?

• Carbonates

• Nitrates

• Sulfides

• Phosphates

What is the solubility status of aluminum carbonate in the reaction?

• Highly soluble

• Insoluble

• Completely soluble

• Slightly soluble

What happens to aluminum carbonate in the reaction?

• It remains unchanged

• It precipitates as a solid

• It forms a gas

• It dissolves completely

What is the purpose of splitting strong electrolytes into ions?

• To write the complete ionic equation

• To balance the equation

• To determine solubility

• To identify the products

Which ions are considered spectator ions in this reaction?

• Nitrate ions

• Aluminum ions

• Hydroxide ions

• Carbonate ions

What is the net charge of the reactants in the net ionic equation?

• Variable

• Zero

• Negative

• Positive

How do you ensure the net ionic equation is balanced?

• By ensuring equal number of atoms and charges

• By checking the solubility

• By removing all ions

• By adding more reactants

What is the final step in writing a net ionic equation?

• Identifying spectator ions

• Checking solubility

• Balancing the molecular equation

• Removing spectator ions

What is the role of Dr. B in the video?

• To discuss the history of chemistry

• To explain the balanced net ionic equation

• To introduce new chemical compounds

• To demonstrate a chemical experiment