Ionic Reactions and Solubility Concepts

This video tutorial explains how to write the net ionic equation for the reaction between barium chloride and sodium carbonate. It begins with balancing the molecular equation, then assigns states to each substance using solubility rules. The tutorial proceeds to break down strong electrolytes into ions for the complete ionic equation and identifies spectator ions to derive the net ionic equation. The final result is the formation of solid barium carbonate as a precipitate.

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

• Determine the solubility of compounds

• Write the complete ionic equation

• Balance the molecular equation

• Identify spectator ions

Which of the following compounds is insoluble in water?

• Barium chloride

• Sodium chloride

• Barium carbonate

• Sodium carbonate

What is the state of sodium chloride in the reaction?

• Solid

• Aqueous

• Liquid

• Gas

What does the 'aq' symbol indicate about a compound?

• It is a solid

• It is a gas

• It is a liquid

• It is dissolved in water

What happens to the precipitate formed in the reaction?

• It falls to the bottom as a solid

• It reacts further with water

• It remains in solution

• It dissolves in water

What is the charge of the carbonate ion?

• 2+

• 1+

• 1-

• 2-

What is the charge of barium in the ionic equation?

• 2-

• 1-

• 1+

• 2+

Which ions are considered spectator ions in this reaction?

• Barium and sodium ions

• Sodium and chloride ions

• Barium and carbonate ions

• Carbonate and chloride ions

Why do we not split apart solids in net ionic equations?

• They do not dissolve in water

• They are not reactive

• They are already balanced

• They are spectator ions

What is the net ionic equation for the reaction between barium chloride and sodium carbonate?

• 2Na+ + 2Cl- → 2NaCl

• BaCl2 + Na2CO3 → BaCO3 + 2NaCl

• Ba2+ + CO3 2- → BaCO3

• Ba2+ + 2Cl- + 2Na+ + CO3 2- → BaCO3 + 2Na+ + 2Cl-