Net Ionic Equations and Solubility

This video tutorial explains how to write and balance the net ionic equation for the reaction between nickel nitrate and sodium carbonate. It covers balancing the molecular equation, determining the solubility and states of substances, forming the complete ionic equation, and deriving the net ionic equation by removing spectator ions. The tutorial emphasizes the importance of charge conservation and balancing atoms in the final net ionic equation.

What is the first step in balancing the molecular equation for a reaction?

• Write the net ionic equation

• Balance the number of atoms on each side

• Determine the solubility of compounds

• Identify the spectator ions

Which of the following is generally soluble in water?

• Nickel carbonate

• Sodium nitrate

• Lead chloride

• Calcium sulfate

Which compound forms a precipitate in the reaction?

• Nickel nitrate

• Sodium nitrate

• Nickel carbonate

• Sodium carbonate

What is the role of solubility rules in writing ionic equations?

• To determine the charge of ions

• To identify spectator ions

• To predict the states of compounds

• To balance the equation

What is the charge of the nickel ion in the reaction?

• 2+

• 1+

• 3+

• 0

Why do we not split solids into ions in the net ionic equation?

• Solids are always spectator ions

• Solids are not part of the reaction

• Solids do not have a charge

• Solids do not dissolve in water

What is the purpose of removing spectator ions in the ionic equation?

• To balance the equation

• To simplify the equation

• To identify the precipitate

• To determine solubility

Which ions are considered spectator ions in this reaction?

• Nickel ions

• Nitrate ions

• Carbonate ions

• Sodium ions

What is the net charge on both sides of a balanced net ionic equation?

• Positive

• Negative

• Zero

• Depends on the reaction

What ensures that the net ionic equation is correctly balanced?

• Equal number of atoms on both sides

• Equal number of molecules on both sides

• Equal number of ions on both sides

• Equal number of compounds on both sides