Net Ionic Equations and Electrolytes

The video tutorial explains how to balance a net ionic equation for magnesium hydroxide and hydrofluoric acid. It begins by balancing the molecular equation, ensuring the correct number of atoms on each side. The states of each substance are identified, noting which are solids, liquids, or aqueous. The tutorial then discusses splitting strong electrolytes into ions to form the complete ionic equation, while weak electrolytes and solids remain intact. The final balanced net ionic equation is presented, highlighting the importance of not splitting weak acids, solids, or liquids.

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

• Split the strong electrolytes

• Determine the states of substances

• Balance the molecular equation

• Identify the spectator ions

How many hydrogens are present on the reactant side after balancing the molecular equation?

• Four

• Three

• Two

• Five

What is the state of magnesium hydroxide in the reaction?

• Liquid

• Gas

• Solid

• Aqueous

Which of the following is considered a weak acid in the reaction?

• Hydrofluoric acid

• Magnesium hydroxide

• Magnesium fluoride

• Water

Why don't we split HF in the complete ionic equation?

• It is a strong acid

• It is a weak electrolyte

• It is a gas

• It is a solid

Which substances are not split into ions in the complete ionic equation?

• Gases

• Liquids

• Strong acids

• Weak acids and solids

What is the final form of the net ionic equation?

• Only solids and liquids split

• No substances split

• Only strong electrolytes split

• All substances split into ions

Why can't magnesium fluoride be split in the net ionic equation?

• It is a solid

• It is a strong electrolyte

• It is a liquid

• It is a gas

What is the role of water in the net ionic equation?

• It is split into ions

• It remains as a liquid

• It is a strong electrolyte

• It is a weak acid

What is the significance of not splitting liquids in net ionic equations?

• They are gases

• They are weak acids

• They are strong electrolytes

• They do not dissociate