Net Ionic Equations and Reactions

This video tutorial explains how to balance the net ionic equation for the reaction between barium carbonate and nitric acid. It covers the steps to balance the molecular equation, determine the states of substances, and write the complete ionic equation. The tutorial also demonstrates how to identify and remove spectator ions to derive the net ionic equation, ensuring charge and atom balance.

What type of reaction occurs between barium carbonate and nitric acid?

• Synthesis

• Decomposition

• Double displacement

• Single displacement

What is the first step in balancing the molecular equation for the reaction?

• Adjusting the coefficients of the products

• Balancing the charges

• Writing the net ionic equation

• Ensuring the number of atoms of each element is equal on both sides

Which of the following is true about barium carbonate in the reaction?

• It dissociates into ions

• It is a strong acid

• It is insoluble and starts as a solid

• It is soluble in water

What is the state of nitric acid in the reaction?

• Aqueous

• Solid

• Liquid

• Gas

Which ions are considered spectator ions in this reaction?

• Nitrate ions

• Hydrogen ions

• Barium ions

• Carbonate ions

What is the purpose of identifying spectator ions in a reaction?

• To balance the equation

• To simplify the net ionic equation

• To find the limiting reactant

• To determine the reaction type

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

• 1+

• 2+

• 1-

• 2-

In the net ionic equation, what happens to the spectator ions?

• They are included in the equation

• They are removed from the equation

• They change their charge

• They form a precipitate

What ensures that the net ionic equation is correctly balanced?

• Equal number of molecules on both sides

• Presence of spectator ions

• Equal number of atoms and charges on both sides

• Formation of a gas

What is the final product of the decomposition of carbonic acid in the reaction?

• Nitrate ions

• Carbon dioxide and water

• Nitric acid

• Barium carbonate