Net Ionic Equations and Solubility

The video tutorial explains how to write a balanced net ionic equation for the reaction between ammonium carbonate and strontium chloride. It begins with balancing the molecular equation, followed by determining the solubility and states of the compounds involved. The tutorial then demonstrates how to form the complete ionic equation and derive the net ionic equation by removing spectator ions. Finally, it concludes with a discussion on charge conservation and the final net ionic equation.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

Which of the following compounds is generally insoluble?

• Ammonium chloride

• Potassium chloride

• Sodium carbonate

• Strontium carbonate

What happens to insoluble compounds in a reaction?

• They evaporate

• They dissolve completely

• They remain as ions

• They form a precipitate

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

• To determine the states of compounds

• To calculate the reaction rate

• To identify spectator ions

• To balance the equation

What is the charge of the ammonium ion?

• 1+

• 1-

• 2+

• 2-

In the complete ionic equation, which ion is not split apart?

• Strontium carbonate

• Ammonium ion

• Chloride ion

• Strontium ion

What is the purpose of identifying spectator ions?

• To calculate the reaction rate

• To determine solubility

• To simplify the net ionic equation

• To balance the equation

What is the net charge on the left side of the net ionic equation?

• 2+

• 0

• 1-

• 2-

Why is it important to ensure the net charge is zero in the final equation?

• To determine solubility

• To calculate the reaction rate

• To identify spectator ions

• To confirm the reaction is balanced

Which ion is typically written first in a net ionic equation?

• Spectator ion

• Negative ion

• Positive ion

• Neutral compound