Net Ionic Equations and Reactions

The video tutorial explains how to write a balanced net ionic equation for the reaction between iron(III) nitrate and hydrochloric acid. It begins by balancing the molecular equation, then assigns states to each substance using solubility rules. The tutorial identifies ions in the solution and highlights that all ions are spectator ions, leading to the conclusion that no reaction occurs. The video emphasizes understanding solubility rules and the concept of spectator ions in net ionic equations.

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

• Write the net ionic equation directly

• Determine the states of substances

• Identify spectator ions

• Balance the molecular equation

What is the chemical formula for iron(III) nitrate?

• Fe3(NO3)2

• Fe2(NO3)3

• Fe(NO3)3

• Fe(NO3)2

How many nitrate ions are present in the balanced molecular equation?

• Four

• Two

• Three

• One

According to solubility rules, what is the state of nitrates in a solution?

• Aqueous

• Gas

• Liquid

• Solid

What is the state of hydrochloric acid in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

What happens to the ions in the solution during the reaction?

• They react to form a new compound

• They evaporate

• They remain unchanged

• They form a precipitate

What are spectator ions?

• Ions that do not change during the reaction

• Ions that form a precipitate

• Ions that participate in the reaction

• Ions that evaporate

What is the net ionic equation for the reaction between Fe(NO3)3 and HCl?

• Fe3+ + 3NO3- → Fe(NO3)3

• No net ionic equation

• 3H+ + 3NO3- → 3HNO3

• Fe3+ + 3Cl- → FeCl3

Why is there no net ionic equation for the reaction?

• All ions form a solid

• All ions react to form a new compound

• All ions are gases

• All ions are spectator ions

What is the final conclusion about the reaction between Fe(NO3)3 and HCl?

• A gas is released

• A new compound is formed

• A precipitate is formed

• No reaction occurs