Net Ionic Equations and Electrolytes

The video tutorial explains how to write the balanced net ionic equation for the reaction between hydrochloric acid (HCl) and zinc sulfide (ZnS). It begins by balancing the molecular equation, then discusses the states of each substance, considering solubility rules. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into ions. Finally, it derives the net ionic equation by removing spectator ions, ensuring that both charge and atoms are balanced.

What is the main goal of the video tutorial?

• To learn about the periodic table

• To write a balanced net ionic equation for HCl and ZnS

• To understand the properties of zinc

• To explore the uses of hydrochloric acid

What is the first step in balancing the molecular equation?

• Balancing the chlorines

• Balancing the zincs

• Balancing the sulfurs

• Balancing the hydrogens

What state is assigned to hydrochloric acid in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

Why is zinc sulfide considered a solid in the net ionic equation?

• It is highly soluble

• It is a strong electrolyte

• It is only slightly soluble

• It is a gas

Which of the following is a weak electrolyte in the reaction?

• HCl

• ZnS

• H2S

• ZnCl2

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

• 1+

• 2-

• 1-

• 2+

Which ions are considered spectator ions in this reaction?

• Sulfide ions

• Chloride ions

• Zinc ions

• Hydrogen ions

What is the purpose of removing spectator ions?

• To simplify the equation

• To balance the equation

• To change the reaction

• To increase the reaction rate

What must be balanced in the net ionic equation?

• Only the atoms

• Neither atoms nor charges

• Only the charges

• Both atoms and charges

What is the key realization about H2S in the net ionic equation?

• It is a gas

• It remains undissociated

• It is a strong electrolyte

• It is a strong acid