Net Ionic Equations and Solubility

The video tutorial explains how to write a balanced net ionic equation for the reaction between copper(II) chloride and ammonium phosphate. It begins with balancing the molecular equation, followed by determining the states of each compound 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 removed to derive the net ionic equation, ensuring both atoms and charges are balanced.

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

• Write the complete ionic equation

• Balance the molecular equation

• Identify spectator ions

• Determine the solubility of compounds

Which of the following compounds is generally insoluble?

• Chlorides

• Ammonium compounds

• Nitrates

• Phosphates

What is the state of copper(II) phosphate in the reaction?

• Solid

• Aqueous

• Gas

• Liquid

What happens to insoluble compounds in a reaction?

• They remain unchanged

• They precipitate as a solid

• They dissolve completely

• They form a gas

What do you do after writing the complete ionic equation?

• Check for charge balance

• Balance the molecular equation

• Identify and remove spectator ions

• Determine the solubility of compounds

Which of the following is a strong electrolyte?

• Ammonium chloride

• Carbon dioxide

• Water

• Copper(II) phosphate

Which ions are considered spectator ions in this reaction?

• Copper ions

• Phosphate ions

• Chloride ions

• Hydrogen ions

Why is it important to remove spectator ions?

• To determine solubility

• To identify the precipitate

• To balance the equation

• To simplify the equation

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

• Positive

• Negative

• Zero

• Variable

What is the final step in verifying the net ionic equation?

• Check for solubility

• Identify spectator ions

• Ensure all compounds are aqueous

• Verify balance of atoms and charge