Net Ionic Equations and Solubility

The video tutorial explains how to write a net ionic equation for the reaction between silver nitrate (AgNO3) and potassium chloride (KCl). It covers the steps of writing a balanced molecular equation, determining the solubility states of the reactants and products, splitting soluble compounds into ions, and identifying spectator ions. The tutorial concludes with the final net ionic equation, emphasizing the importance of understanding solubility rules and ionic charges.

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

• Split compounds into ions

• Determine the solubility of compounds

• Identify spectator ions

• Write the balanced molecular equation

Which of the following is generally soluble in water?

• Potassium chloride

• Silver chloride

• Lead sulfate

• Calcium carbonate

What is the solubility of silver chloride (AgCl) in water?

• Highly soluble

• Partially soluble

• Insoluble

• Soluble

Which ion does potassium (K) form in solution?

• K2-

• K+

• K2+

• K-

What is the charge on the nitrate ion (NO3)?

• 1-

• 2+

• 2-

• 1+

Which of the following compounds will not be split into ions in the complete ionic equation?

• Silver nitrate (AgNO3)

• Silver chloride (AgCl)

• Potassium chloride (KCl)

• Potassium nitrate (KNO3)

What are spectator ions?

• Ions that are only present in the reactants

• Ions that do not participate in the reaction

• Ions that form a precipitate

• Ions that change their oxidation state

Which ions are considered spectator ions in the reaction between AgNO3 and KCl?

• Ag+ and Cl-

• K+ and NO3-

• Ag+ and NO3-

• K+ and Cl-

What is the net ionic equation for the reaction between AgNO3 and KCl?

• Ag+ + NO3- → AgNO3

• Ag+ + Cl- → AgCl

• Ag+ + NO3- + K+ + Cl- → AgCl + KNO3

• AgNO3 + KCl → AgCl + KNO3

What does the net ionic equation represent?

• The solubility of the compounds

• The balanced molecular equation

• Only the ions that participate in forming the precipitate

• All ions present in the solution