Net Ionic Equations and Reactions

The video explores the net ionic equation for the reaction between sodium chloride and sulfuric acid. Initially, it assumes both are in aqueous solutions, leading to no reaction as all compounds remain dissociated into ions. An alternative scenario with solid sodium chloride and liquid sulfuric acid is discussed, but it presents challenges in writing a net ionic equation due to the presence of solids, liquids, and gases, which are not split into ions. The video concludes that a net ionic equation cannot be written for this reaction.

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

• Gas

• Liquid

• Solid

• Aqueous

What is the state of sulfuric acid when it dissociates in water?

• Gas

• Solid

• Liquid

• Aqueous

Why does no reaction occur when sodium chloride and sulfuric acid are both in aqueous form?

• They react to form a gas.

• They form a new compound.

• All ions remain dissociated.

• They form a precipitate.

What happens to the ions in the reaction between aqueous sodium chloride and sulfuric acid?

• They form a gas.

• They form a new compound.

• They remain unchanged.

• They precipitate out.

What is the role of sodium in the reaction with sulfuric acid?

• It forms a new compound.

• It reacts to form a gas.

• It remains as an ion.

• It forms a precipitate.

In the alternative scenario, what state does hydrochloric acid end up in?

• Solid

• Liquid

• Aqueous

• Gas

What is the result of starting with solid sodium chloride and liquid sulfuric acid?

• Formation of a gas and a solid.

• No reaction occurs.

• Formation of a new liquid.

• Formation of an aqueous solution.

Why can't solids be split in net ionic equations?

• They react too quickly.

• They are already dissociated.

• They do not dissolve in water.

• They do not form ions.

What is the main challenge in writing a net ionic equation for this reaction?

• The reaction is too fast.

• Too many ions are formed.

• Lack of reactants.

• Presence of solids, liquids, and gases.

Why can't a net ionic equation be written for this reaction?

• The reactants are not soluble.

• No ions are formed.

• The reaction is too slow.

• The products are unknown.