Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between chloric acid (HClO3) and barium hydroxide (Ba(OH)2). It begins with balancing the molecular equation, assigning states to each substance, and dissociating strong acids and bases. The complete ionic equation is formed, and spectator ions are identified and removed. The final net ionic equation is simplified, ensuring that charges and atoms are balanced.

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

• Write the complete ionic equation

• Determine the states of substances

• Balance the molecular equation

• Identify spectator ions

How do you balance the chlorate ions in the reaction between HClO3 and Ba(OH)2?

• Add a coefficient of 3 in front of Ba(OH)2

• Add a coefficient of 2 in front of HClO3

• Add a coefficient of 2 in front of BaClO3

• Add a coefficient of 3 in front of HClO3

What is the state of chloric acid in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

Which of the following is considered a strong base in the reaction?

• HClO3

• Ba(OH)2

• BaClO3

• H2O

What is the purpose of identifying spectator ions in a reaction?

• To balance the equation

• To simplify the equation

• To determine the states of substances

• To calculate the net charge

Which ions are considered spectator ions in this reaction?

• Hydrogen ions

• Barium ions

• Chlorate ions

• Hydroxide ions

What is the net charge of the final net ionic equation?

• Zero

• Undefined

• Negative

• Positive

Why do we reduce coefficients in the final net ionic equation?

• To simplify the equation

• To balance the charges

• To identify spectator ions

• To match the molecular equation

What is the net ionic equation for the reaction between HClO3 and Ba(OH)2?

• HClO3 + Ba(OH)2 → BaClO3 + H2O

• 2HClO3 + Ba(OH)2 → BaClO3 + 2H2O

• H+ + OH- → H2O

• 2H+ + 2OH- → 2H2O

What ensures that the charges are balanced in the net ionic equation?

• The net charge of zero

• The dissociation of strong acids

• The presence of spectator ions

• The reduction of coefficients