Net Ionic Equations and Solubility

The video tutorial explains how to balance the net ionic equation for the reaction between potassium phosphate (K3PO4) and silver nitrate (AgNO3). It begins by balancing the molecular equation, then discusses the solubility and states of the reactants and products. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into ions. Finally, it derives the net ionic equation by removing spectator ions and ensuring charge and atom balance.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

Why is potassium phosphate considered soluble in this reaction?

• Because it reacts with silver nitrate

• Because it forms a precipitate

• Because potassium compounds are generally soluble

• Because all phosphates are soluble

What is the state of silver phosphate in the reaction?

• Gas

• Solid

• Aqueous

• Liquid

What is the significance of a precipitate in a chemical reaction?

• It means the reaction is endothermic

• It suggests the reaction is reversible

• It shows that a solid is formed from the reaction

• It indicates a gas is formed

Why are nitrates generally considered soluble?

• They form weak bases

• They form strong acids

• They are always gases

• They dissolve easily in water

What is the charge of a potassium ion in the complete ionic equation?

• 2+

• 1+

• 1-

• 3+

What is the role of the periodic table in determining ion charges?

• It helps identify the number of neutrons

• It provides the atomic mass

• It indicates the typical charge of elements

• It shows the electron configuration

Which ions are considered spectator ions in this reaction?

• Silver ions and phosphate ions

• Potassium ions and nitrate ions

• Silver ions and nitrate ions

• Potassium ions and phosphate ions

What is the net ionic equation for the reaction between potassium phosphate and silver nitrate?

• 3K+ + 3NO3^- → 3KNO3

• K3PO4 + 3AgNO3 → 3KNO3 + Ag3PO4

• 3Ag+ + PO4^3- → Ag3PO4

• 3K+ + PO4^3- + 3Ag+ + 3NO3^- → 3K+ + 3NO3^- + Ag3PO4

How is charge conservation demonstrated in the net ionic equation?

• The total charge on both sides is zero

• The total charge is not conserved

• The total charge on both sides is positive

• The total charge on both sides is negative