Electrolysis of Aqueous Solutions

The video tutorial covers the electrolysis of aqueous solutions, starting with a refresher on electrolysis, which involves splitting compounds using electricity. It explains how ions in aqueous solutions can move freely, allowing electrolysis to occur. The video details reactions at the cathode and anode, highlighting the discharge of ions based on reactivity. Case studies of copper sulfate and sodium chloride solutions illustrate these principles, showing how different ions are discharged to form specific products. The tutorial concludes with a summary of key reactions and outcomes in electrolysis.

What is the primary purpose of electrolysis?

• To cool compounds using electricity

• To heat compounds using electricity

• To split compounds using electricity

• To combine elements using electricity

Why can aqueous solutions be electrolyzed?

• Because solids conduct electricity better

• Because water is a good insulator

• Because ions can move freely

• Because ions are fixed in place

What happens at the cathode if the metal is less reactive than hydrogen?

• Hydrogen gas is formed

• The metal is deposited

• Oxygen gas is formed

• The metal dissolves

What is formed at the anode when halide ions are present?

• Oxygen gas

• Water

• Hydrogen gas

• Halogen gas

In the electrolysis of copper sulfate, what is formed at the cathode?

• Copper metal

• Hydrogen gas

• Chlorine gas

• Oxygen gas

During the electrolysis of sodium chloride, what is formed at the anode?

• Hydrogen gas

• Sodium metal

• Chlorine gas

• Oxygen gas

What determines whether hydrogen or a metal is discharged at the cathode?

• The reactivity of the metal

• The concentration of the solution

• The color of the solution

• The temperature of the solution