Net Ionic Equations and Solubility

The video tutorial explains how to write a balanced net ionic equation for the reaction between ammonium carbonate and barium hydroxide. It begins with balancing the molecular equation and identifying the states of each substance, highlighting the solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation, noting that solids, gases, and liquids remain intact. Since there are no spectator ions, the complete ionic equation is the same as the net ionic equation. The video concludes by ensuring charge and atom balance, with a brief discussion on ammonia's behavior as a weak electrolyte.

What is the first step in writing the net ionic equation for ammonium carbonate and barium hydroxide?

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

Why is ammonium carbonate considered soluble?

• Because it forms a precipitate

• Because ammonium compounds are generally soluble

• Because all carbonates are soluble

• Because it is a strong acid

What is the state of barium carbonate in the reaction?

• Liquid

• Solid

• Gas

• Aqueous

How is ammonia treated in the net ionic equation?

• As a strong electrolyte

• As a weak electrolyte

• As a solid

• As a spectator ion

What is the state of water in the reaction?

• Gas

• Liquid

• Solid

• Aqueous

Which substances are not split into ions in the complete ionic equation?

• All reactants

• All products

• Strong acids

• Solids, gases, and liquids

Why are there no spectator ions in this reaction?

• All ions are the same in reactants and products

• The reaction does not involve ions

• Spectator ions are not considered

• All ions are different in reactants and products

What is conserved in the net ionic equation?

• Neither mass nor charge

• Charge only

• Mass only

• Both mass and charge

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

• Variable

• Zero

• Negative

• Positive

How is ammonia described in terms of its electrolytic nature?

• Strong base

• Weak electrolyte

• Non-electrolyte

• Strong acid