Net Ionic Equations and Ammonium Compounds

This video tutorial explains how to write a balanced net ionic equation for the reaction between ammonium nitrate and sodium hydroxide. It covers balancing the molecular equation, determining the states of substances using solubility rules, and splitting strong electrolytes into ions to form the complete ionic equation. The tutorial then demonstrates how to identify and cross out spectator ions to derive the net ionic equation, ensuring charge conservation and balanced atoms. The video concludes with a discussion on the implications of ammonia being a weak base and the importance of charge neutrality.

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

• Write the complete ionic equation

• Balance the molecular equation

• Identify spectator ions

• Determine the states of the compounds

Which of the following is true about compounds with the ammonium ion?

• They are weak bases

• They are very soluble

• They are gases

• They are insoluble

What is the state of sodium hydroxide in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

Why is ammonia not split into ions in the complete ionic equation?

• It is a solid

• It is a strong acid

• It is a weak electrolyte

• It is a strong base

What is the charge of the ammonium ion?

• 1-

• 1+

• 2-

• 2+

Which ions are considered spectator ions in this reaction?

• Ammonia and water

• Ammonium and hydroxide

• Sodium and nitrate

• Hydroxide and water

What is the net ionic equation derived from the reaction?

• NH3 + H2O → NH4+ + OH-

• NH4+ + OH- → NH3 + H2O

• Na+ + NO3- → NaNO3

• NH4NO3 + NaOH → NaNO3 + NH3 + H2O

What is conserved in a balanced net ionic equation?

• Neither mass nor charge

• Both mass and charge

• Only charge

• Only mass

What happens to the charge of the compounds in the net ionic equation?

• It becomes positive

• It becomes negative

• It remains neutral

• It doubles

If ammonia was aqueous, what would be its state symbol?

• s

• aq

• g

• l