Net Ionic Equations and Solubility

This video tutorial guides viewers through balancing the net ionic equation for the reaction between sodium phosphate (Na3PO4) and magnesium chloride (MgCl2). It begins with balancing the molecular equation, then discusses the solubility of the compounds involved, identifying which are soluble and which form a precipitate. The tutorial proceeds to break down the compounds into their respective ions to form the complete ionic equation. Finally, it demonstrates how to derive the net ionic equation by eliminating spectator ions and ensuring both charge and mass are balanced.

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

• Identify spectator ions

• Balance the molecular equation

• Write the complete ionic equation

• Check for charge balance

Which of the following compounds is typically insoluble in water?

• Ammonium sulfate

• Sodium chloride

• Magnesium phosphate

• Potassium nitrate

What happens to magnesium phosphate in the reaction?

• It reacts with sodium ions

• It evaporates

• It dissolves in water

• It forms a precipitate

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

• 1-

• 2-

• 3-

• 4-

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

• Eight

• Two

• Four

• Six

What is the role of spectator ions in a chemical reaction?

• They balance the equation

• They change the state of the reaction

• They participate in the reaction

• They remain unchanged and do not participate

Which ions are removed to form the net ionic equation?

• Hydrogen and oxygen ions

• Potassium and nitrate ions

• Magnesium and phosphate ions

• Sodium and chloride ions

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

• Zero

• Negative

• Positive

• Variable

Why is it important to ensure mass balance in a chemical equation?

• To change the reaction pathway

• To increase reaction speed

• To satisfy the law of conservation of mass

• To conserve energy

What is the significance of balancing charges in a net ionic equation?

• To ensure the reaction is spontaneous

• To maintain electrical neutrality

• To increase solubility

• To change the reaction rate