Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between calcium hydroxide and nitrous acid. It covers balancing the molecular equation, assigning states to substances, splitting strong electrolytes into ions, and identifying spectator ions. The tutorial concludes with the final net ionic equation, ensuring charge and atom balance.

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

• Write the states of each substance

• Identify spectator ions

• Balance the molecular equation

• Split all compounds into ions

How many nitrite ions are present after balancing the molecular equation?

• One

• Four

• Two

• Three

Why is nitrous acid not split into ions in the net ionic equation?

• It is a strong acid

• It is a weak acid

• It is a gas

• It is a solid

Which of the following is not split into ions in the net ionic equation?

• All are split into ions

• Calcium nitrite

• Nitrous acid

• Calcium hydroxide

What is the role of spectator ions in a net ionic equation?

• They change the charge balance

• They participate in the reaction

• They are removed from the equation

• They are the main reactants

Which ion is identified as a spectator ion in this reaction?

• Hydrogen ion

• Calcium ion

• Nitrite ion

• Hydroxide ion

What must be conserved in a balanced net ionic equation?

• Both mass and charge

• Neither mass nor charge

• Charge only

• Mass only

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

• Reducing coefficients to their simplest form

• Adding more reactants

• Changing the states of substances

• Removing all ions

Why is it important to ensure the charge is the same on both sides of the equation?

• To find the limiting reactant

• To balance the equation

• To identify spectator ions

• To determine solubility

What is the significance of not writing the coefficient '1' in the final equation?

• It simplifies the equation

• It indicates a strong acid

• It highlights the main reactant

• It shows the reaction is complete