Net Ionic Equations and Reactions

The video tutorial explains how to write a balanced net ionic equation for the reaction between chloric acid (HClO3) and sodium hydroxide (NaOH). It begins by balancing the molecular equation and determining the states of each substance. 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 emphasizing the conservation of charge and mass in the balanced equation.

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

• Split the electrolytes into ions

• Identify spectator ions

• Balance the molecular equation

• Write the states of substances

Which of the following is considered a strong acid in the video?

• H2O

• NaClO3

• NaOH

• HClO3

What is the state of sodium chlorate in the reaction?

• Liquid

• Aqueous

• Solid

• Gas

What is the charge of the hydroxide ion?

• 1+

• 2+

• 2-

• 1-

Which ions are considered spectator ions in this reaction?

• Hydrogen and hydroxide ions

• Sodium and chlorate ions

• Chloride and sodium ions

• Hydrogen and sodium ions

What remains after removing the spectator ions?

• Net ionic equation

• Complete ionic equation

• Molecular equation

• Balanced equation

What is conserved in a balanced net ionic equation?

• Only mass

• Only charge

• Both mass and charge

• Neither mass nor charge

How many hydrogens are present in the products of the net ionic equation?

• One

• Two

• Three

• Four

What is the final product formed in the net ionic equation?

• HClO3

• NaOH

• H2O

• NaClO3

Who is the presenter of the video?

• Dr. D

• Dr. A

• Dr. B

• Dr. C