Net Ionic Equations and Spectator Ions

This video tutorial explains how to write the net ionic equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH). It begins with balancing the molecular equation and identifying the states of the compounds involved. The tutorial then demonstrates how to split strong electrolytes into their respective ions and write the complete ionic equation. Spectator ions are identified and crossed out to derive the net ionic equation. The video concludes with a recap of the steps involved in the process.

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

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

• Write the complete ionic equation

Which of the following is a strong electrolyte?

• CO2

• HCl

• H2O

• NaCl

What is the state of sodium chloride in the reaction?

• Solid

• Liquid

• Aqueous

• Gas

What charge does a sodium ion (Na+) have?

• 2+

• 1-

• 2-

• 1+

Which ion is not split into its components in the ionic equation?

• OH-

• H2O

• Cl-

• Na+

What are spectator ions?

• Ions that form a precipitate

• Ions that are gases

• Ions that participate in the reaction

• Ions that do not change during the reaction

Which ions are removed to form the net ionic equation?

• All ions

• Ions that form a gas

• Only the ions that form a solid

• Spectator ions

What is the net ionic equation for the reaction between HCl and NaOH?

• H2O → H+ + OH-

• H+ + OH- → H2O

• Na+ + Cl- → NaCl

• HCl + NaOH → NaCl + H2O

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

• Balancing the molecular equation

• Writing the states of reactants

• Crossing out spectator ions

• Determining the charges of ions

What is the purpose of writing a net ionic equation?

• To determine the solubility of compounds

• To balance the chemical equation

• To highlight the ions that participate in the reaction

• To show all reactants and products