Net Ionic Equations and Electrolytes

This video tutorial explains how to write the balanced net ionic equation for the reaction between sulfuric acid (H2SO4) and zinc sulfide (ZnS). It begins with balancing the molecular equation, then identifies the states of each substance. The tutorial proceeds to write the complete ionic equation by splitting strong electrolytes into ions. Finally, it derives the net ionic equation by removing spectator ions, ensuring charge and atom balance. The video emphasizes understanding solubility rules and the properties of strong and weak electrolytes.

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

• Split strong electrolytes into ions

• Identify spectator ions

• Balance the molecular equation

• Determine the states of substances

Which of the following is a strong electrolyte?

• Water

• H2S

• Sulfuric acid

• Zinc sulfide

What state is zinc sulfide in during the reaction?

• Gas

• Liquid

• Aqueous

• Solid

Why do we not split solids in net ionic equations?

• They are already balanced

• They are weak electrolytes

• They do not dissolve in water

• They are spectator ions

What charge does the zinc ion have in the reaction?

• 1+

• 2+

• 1-

• 2-

Which ion is identified as a spectator ion in this reaction?

• Sulfate ion

• Hydrogen ion

• Sulfide ion

• Zinc ion

What is the purpose of identifying spectator ions?

• To find the limiting reactant

• To balance the equation

• To determine solubility

• To simplify the net ionic equation

What is conserved in a balanced net ionic equation?

• Charge only

• Mass only

• Neither mass nor charge

• Both mass and charge

How do you verify that a net ionic equation is balanced?

• Check the solubility of products

• Identify all spectator ions

• Count the number of atoms and charges

• Ensure all reactants are used

What is the final product of the reaction between sulfuric acid and zinc sulfide?

• Zinc sulfate and hydrogen sulfide

• Zinc nitrate and hydrogen gas

• Zinc oxide and sulfur dioxide

• Zinc chloride and water