Net Ionic Equations and Solubility

This video tutorial explains how to write a balanced net ionic equation for the reaction between lead(II) nitrate and sodium phosphate. It begins with balancing the molecular equation, followed by determining the states of each substance using solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Finally, it identifies and removes spectator ions to derive the net ionic equation, emphasizing the formation of lead(II) phosphate as a precipitate.

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

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

• Identify spectator ions

Which of the following is generally soluble in water?

• Lead(II) phosphate

• Sodium compounds

• Phosphates

• Carbonates

What is the charge of a nitrate ion?

• 1-

• 2+

• 1+

• 3-

How many sodium ions are present in the complete ionic equation for this reaction?

• Four

• Three

• Six

• Two

What do we call ions that do not participate in the net ionic equation?

• Active ions

• Spectator ions

• Soluble ions

• Precipitate ions

Which ions are crossed out when deriving the net ionic equation?

• Ions that are aqueous

• Ions that appear on both sides of the equation

• Ions that are insoluble

• Ions that form a solid

What is the final product formed in the reaction between lead(II) nitrate and sodium phosphate?

• Sodium nitrate

• Sodium phosphate

• Lead(II) nitrate

• Lead(II) phosphate

What is the state of lead(II) phosphate in the net ionic equation?

• Solid

• Liquid

• Gas

• Aqueous

Which of the following is NOT a spectator ion in this reaction?

• Lead(II) ion

• Nitrate ion

• Sodium ion

• Phosphate ion

What is the purpose of writing a net ionic equation?

• To show all ions present in a solution

• To highlight the formation of precipitates

• To balance the molecular equation

• To identify the most reactive ions