Net Ionic Equations and Solubility

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between calcium nitrate and sodium sulfide. It begins with balancing the molecular equation, then moves on to determining the states of substances using solubility rules. The tutorial explains how to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring the conservation of charge and atom balance in the final equation.

What is the first step in balancing net ionic equations?

• Identify spectator ions

• Balance the molecular equation

• Write the states of substances

• Split strong electrolytes into ions

Which of the following is generally soluble according to solubility rules?

• Lead sulfide

• Calcium sulfide

• Silver chloride

• Sodium compounds

What happens to calcium sulfide in the reaction?

• It forms a precipitate

• It dissolves in water

• It reacts with sodium

• It remains as ions

What is the charge of a calcium ion in the complete ionic equation?

• 2+

• 2-

• 1+

• 1-

Which ions are not split in the net ionic equation?

• Sulfide ions

• Nitrate ions

• Sodium ions

• Calcium sulfide

What are spectator ions?

• Ions that form a precipitate

• Ions that do not change during the reaction

• Ions that are not present in the products

• Ions that participate in the reaction

Which ions are crossed out as spectator ions in this reaction?

• Calcium and nitrate ions

• Sodium and sulfide ions

• Calcium and sulfide ions

• Sodium and nitrate ions

What is the net charge on both sides of the net ionic equation?

• 2-

• 1+

• 2+

• 0

Why is it important to ensure that the net ionic equation is balanced?

• To identify spectator ions

• To ensure the reaction is spontaneous

• To predict the products

• To conserve mass and charge

What is the final product of the reaction between calcium nitrate and sodium sulfide?

• Calcium nitrate

• Sodium nitrate

• Calcium sulfide

• Sodium sulfide