Net Ionic Equations and Spectator Ions

The video tutorial explains how to balance the net ionic equation for the reaction between iron(II) sulfate and potassium hydroxide. It begins by balancing the molecular equation, then discusses the solubility and states of the substances involved. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring the charge and atoms are balanced in the final equation.

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

• Determine the solubility of compounds

• Write the complete ionic equation

• Balance the molecular equation

• Identify spectator ions

Which of the following is generally soluble according to solubility rules?

• Calcium sulfate

• Lead(II) chloride

• Potassium hydroxide

• Iron(II) hydroxide

What is the state of iron(II) hydroxide in the reaction?

• Aqueous

• Liquid

• Gas

• Solid

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

• Magnesium hydroxide

• Calcium hydroxide

• Potassium hydroxide

• Iron(II) hydroxide

What is the role of solubility rules in writing net ionic equations?

• To balance the molecular equation

• To predict the formation of precipitates

• To identify spectator ions

• To determine the charge of ions

What is the charge of the sulfate ion?

• 2-

• 2+

• 1-

• 1+

Which ions are considered spectator ions in this reaction?

• Iron(II) ions

• Hydroxide ions

• Potassium ions

• Sulfate ions

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

• They are included in the final equation

• They are removed from the equation

• They change their charge

• They form a precipitate

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

• 2-

• 2+

• 1+

• 0

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

• To determine the reaction rate

• To verify the conservation of mass and charge

• To confirm the reaction is spontaneous

• To ensure the reaction is endothermic