Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between nitric acid (HNO3) and ammonium hydroxide (NH4OH). It begins with balancing the molecular equation, then determining the states of each substance. The tutorial proceeds to split strong electrolytes into ions for the complete ionic equation and identifies spectator ions to derive the net ionic equation. The video concludes by discussing the conservation of charge and mass in the reaction.

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

• Identify spectator ions

• Balance the molecular equation

• Write the complete ionic equation

• Determine the states of substances

Which of the following is a strong acid that dissociates completely in water?

• HCl

• HNO3

• NH4OH

• H2O

What state symbol is used for substances that are soluble in water?

• (aq)

• (g)

• (s)

• (l)

What is the charge of the nitrate ion (NO3-)?

• 1-

• 2-

• 2+

• 1+

Which ion is not split in the net ionic equation?

• NO3-

• H2O

• H+

• NH4+

What is the purpose of identifying spectator ions?

• To determine solubility

• To simplify the net ionic equation

• To balance the equation

• To find the limiting reactant

Which ions are considered spectator ions in this reaction?

• H+ and OH-

• NH4+ and NO3-

• H2O and NO3-

• NH4+ and OH-

What is conserved in a balanced net ionic equation?

• Neither mass nor charge

• Both mass and charge

• Only charge

• Only mass

How many hydrogen atoms are present on each side of the net ionic equation?

• Two

• One

• Four

• Three

What is the final product in the net ionic equation for the reaction between HNO3 and NH4OH?

• OH-

• NH4+

• NO3-

• H2O