Spectator Ions and Net Ionic Equations

The video tutorial explains how to write a balanced net ionic equation for the reaction between nitric acid (HNO3) and potassium hydroxide (KOH). It begins by introducing the concept of net ionic equations and the neutralization reaction between a strong acid and a strong base. The tutorial then covers balancing the molecular equation and identifying the states of the reactants and products. It discusses the dissociation of strong acids and bases and the solubility rules. The complete ionic equation is written by splitting strong electrolytes into their ions. Finally, the net ionic equation is derived by removing spectator ions, resulting in the formation of water.

What type of reaction occurs between nitric acid and potassium hydroxide?

• Neutralization

• Decomposition

• Precipitation

• Redox

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

• CH3COOH

• H2SO4

• HNO3

• HCl

What is the state of potassium hydroxide in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

Which ion is considered a spectator ion in the reaction?

• Hydrogen ion

• Nitrate ion

• Hydroxide ion

• Water molecule

What is the charge of the nitrate ion in the complete ionic equation?

• +2

• -1

• +1

• -2

In the complete ionic equation, which ion is paired with the hydroxide ion?

• Chloride ion

• Nitrate ion

• Hydrogen ion

• Potassium ion

What remains in the net ionic equation after removing spectator ions?

• K+ and NO3-

• H2O and K+

• H+ and OH-

• NO3- and OH-

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

• H2O

• HNO3

• KNO3

• KOH

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

• KNO3

• HNO3

• KOH

• H2O

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

• To determine the reaction rate

• To simplify the net ionic equation

• To identify the limiting reactant

• To balance the equation