Ionic Equations and Solubility Concepts

The video tutorial explains how to write the balanced net ionic equation for the reaction between iron(III) chloride (FeCl3) and sulfuric acid (H2SO4). It begins with balancing the molecular equation, followed by determining the solubility and states of the compounds involved. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Finally, it identifies spectator ions and presents the balanced net ionic equation, ensuring both atoms and charges are balanced.

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

• Split strong electrolytes into ions

• Balance the molecular equation

• Determine the states of compounds

• Identify spectator ions

How many sulfate ions are present in the balanced molecular equation for FeCl3 and H2SO4?

• One

• Four

• Two

• Three

According to solubility rules, what is the state of sulfuric acid in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

What is the solubility status of iron(III) sulfate in this reaction?

• Insoluble

• Slightly soluble

• Highly soluble

• Completely soluble

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

• 2-

• 1-

• 2+

• 1+

How many hydrogen ions are present in the complete ionic equation?

• Eight

• Six

• Four

• Two

What are spectator ions in a chemical reaction?

• Ions that are gases

• Ions that do not change during the reaction

• Ions that form a precipitate

• Ions that participate in the reaction

Which ions are removed as spectator ions in this reaction?

• Hydrogen ions

• Iron ions

• Sulfate ions

• Chloride ions

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

• Positive

• Variable

• Negative

• Zero

What ensures the net ionic equation is correctly balanced?

• Equal number of atoms only

• Presence of a precipitate

• Both atoms and charges are balanced

• Equal charges only