Net Ionic Equations and Balancing

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between iron(III) sulfate and potassium hydroxide. It begins with balancing the molecular equation, identifying the states of each compound, and then forming the complete ionic equation by splitting strong electrolytes into ions. The tutorial concludes by identifying spectator ions and writing the final net ionic equation, ensuring charge and atom balance on both sides.

What is the main focus of this video tutorial?

• Balancing chemical equations

• Writing the balanced net ionic equation for a reaction

• Understanding the periodic table

• Learning about acids and bases

What is the first step in balancing the molecular equation for the reaction?

• Balancing the iron atoms

• Balancing the hydroxide ions

• Balancing the potassium ions

• Balancing the sulfate ions

Which compound is considered slightly soluble but treated as a solid in the net ionic equation?

• Calcium carbonate

• Sodium chloride

• Iron(III) sulfate

• Potassium hydroxide

What is the state of potassium hydroxide in the reaction?

• Gas

• Aqueous

• Liquid

• Solid

What do you do with strong electrolytes in the complete ionic equation?

• Split them into ions

• Ignore them

• Combine them into compounds

• Convert them to solids

Which ions are considered spectator ions in this reaction?

• Sulfate ions

• Potassium ions

• Hydroxide ions

• Iron ions

What is the charge balance on both sides of the net ionic equation?

• Six positive on both sides

• Six negative on both sides

• Three positive on both sides

• Three negative on both sides

What happens to the spectator ions in the net ionic equation?

• They are converted to solids

• They are included in the final equation

• They are doubled in the equation

• They are removed from the equation

What is the final product that forms as a solid in this reaction?

• Iron(III) hydroxide

• Calcium carbonate

• Sodium chloride

• Potassium sulfate

Why is it important to ensure the charge is balanced in a net ionic equation?

• To prevent the formation of gases

• To make the equation look neat

• To satisfy the law of conservation of mass

• To ensure the reaction is possible