Balancing Chemical Reactions and Ions

This video tutorial explains how to balance the net ionic equation for sodium sulfide reacting with hydrochloric acid. It begins with balancing the molecular equation, then describes the states of each substance, and forms the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring the conservation of charge and atoms in the balanced equation.

What are the products formed when sodium sulfide reacts with hydrochloric acid?

• Sodium sulfide and water

• Sodium sulfate and hydrogen chloride

• Sodium chloride and hydrogen sulfide

• Sodium chloride and hydrogen gas

How many sodium atoms are needed to balance the molecular equation for the reaction of sodium sulfide with hydrochloric acid?

• Four

• Three

• One

• Two

What is the state of sodium chloride when dissolved in water?

• Aqueous

• Gas

• Solid

• Liquid

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

• Na2S

• H2S

• NaCl

• HCl

What is the charge on the sulfide ion in the complete ionic equation?

• 1+

• 2+

• 2-

• 1-

Which ions are considered spectator ions in the reaction between sodium sulfide and hydrochloric acid?

• Sodium and chloride ions

• Chloride and sulfide ions

• Hydrogen and sulfide ions

• Sodium and hydrogen ions

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

• 2+

• 1+

• 1-

• 0

How many hydrogen atoms are present on each side of the balanced net ionic equation?

• Four

• Three

• Two

• One

In the net ionic equation, which compound remains unchanged and is not split into ions?

• H2S

• NaCl

• Na2S

• HCl

Why is it important to ensure that charge is conserved in a net ionic equation?

• To balance the number of atoms

• To ensure the reaction is spontaneous

• To maintain electrical neutrality

• To increase reaction rate