Ionic Equations and Solubility Concepts

The video tutorial explains how to write a balanced net ionic equation for the reaction between calcium chloride and potassium carbonate. It begins with balancing the molecular equation, followed by determining the states of substances using solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and crossed out to derive the net ionic equation. The video concludes by ensuring charge conservation and atom balance in the final equation.

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

• Identify spectator ions

• Balance the molecular equation

• Write the complete ionic equation

• Determine the solubility of compounds

Which of the following is generally insoluble in water?

• Carbonates

• Nitrates

• Potassium compounds

• Chlorides

What is the state of calcium carbonate in the reaction?

• Aqueous

• Gaseous

• Liquid

• Solid

How do you represent calcium ions in the complete ionic equation?

• Ca2-

• Ca+

• Ca2+

• Ca-

What is the charge of the carbonate ion?

• 2-

• 1-

• 2+

• 1+

Why are spectator ions removed from the complete ionic equation?

• They form a precipitate

• They are gases

• They are not involved in the reaction

• They change state during the reaction

Which ions are considered spectator ions in this reaction?

• Calcium and potassium ions

• Calcium and carbonate ions

• Potassium and chloride ions

• Chloride and carbonate ions

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

• 0

• 2-

• 2+

• 1+

What must be conserved in a balanced net ionic equation?

• Only mass

• Both mass and charge

• Neither mass nor charge

• Only charge

What is the final product formed in the reaction between calcium chloride and potassium carbonate?

• Potassium chloride

• Calcium carbonate

• Potassium carbonate

• Calcium chloride