Net Ionic Equations and Solubility

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between barium nitrate and sodium phosphate. It begins with balancing the molecular equation, followed by determining the states of each substance using solubility rules. The tutorial then explains how to write the complete ionic equation by splitting strong electrolytes into ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes with verifying the equation by ensuring charge and atom balance.

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

• Balance the molecular equation

• Identify spectator ions

• Determine the states of substances

• Write the complete ionic equation

Which of the following is generally soluble in water?

• Sodium compounds

• Barium phosphate

• Carbonates

• Phosphates

What happens to barium phosphate in the reaction?

• It remains as ions

• It reacts with sodium

• It forms a precipitate

• It dissolves in water

What is the charge of a nitrate ion?

• 1+

• 2+

• 1-

• 3-

How many barium ions are present in the complete ionic equation?

• Four

• Three

• One

• Two

Which group on the periodic table does barium belong to?

• Group 1

• Group 4

• Group 2

• Group 3

Which ions are considered spectator ions in this reaction?

• Hydroxide ions

• Sodium ions

• Phosphate ions

• Barium ions

What is the purpose of removing spectator ions?

• To balance the equation

• To simplify the net ionic equation

• To determine solubility

• To identify reactants

What is the net charge of the final net ionic equation?

• 1-

• 3-

• 2+

• 0

What ensures the net ionic equation is correct?

• Presence of spectator ions

• Balanced charge only

• Balanced atoms and charge

• Balanced atoms only