Net Ionic Equations and Solubility

This video tutorial guides viewers through the process of balancing a net ionic equation for the reaction between potassium carbonate and zinc nitrate. It begins with balancing the molecular equation, then determining the states of each substance, and proceeds to split strong electrolytes into their ions to form the complete ionic equation. Finally, the video explains how to derive the net ionic equation by removing spectator ions, ensuring charge and atom balance, and concludes with a brief discussion on the presentation of ions.

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

• Identify spectator ions

• Balance the molecular equation

• Split compounds into ions

• Determine the solubility of compounds

Why is a coefficient of 2 added to zinc nitrate in the molecular equation?

• To balance the zinc atoms

• To balance the nitrate ions

• To balance the potassium ions

• To balance the carbonate ions

Which of the following compounds is typically insoluble?

• Potassium nitrate

• Zinc nitrate

• Potassium carbonate

• Zinc carbonate

What is the charge of a potassium ion?

• 1-

• 1+

• 2-

• 2+

In the complete ionic equation, which ion is not split into its components?

• Potassium ion

• Nitrate ion

• Carbonate ion

• Zinc carbonate

What is the purpose of identifying spectator ions?

• To determine solubility

• To find the charge balance

• To simplify the net ionic equation

• To balance the equation

Which ions are considered spectator ions in this reaction?

• Carbonate ions

• Zinc ions

• Zinc and carbonate ions

• Potassium and nitrate ions

What is conserved in a balanced net ionic equation?

• Neither mass nor charge

• Both mass and charge

• Only charge

• Only mass

Why might the positive ion be written first in the net ionic equation?

• It changes the solubility

• It affects the reaction

• It looks more organized

• It is a requirement

What is the final net ionic equation for the reaction between potassium carbonate and zinc nitrate?

• 2K+ + 2NO3^- → 2KNO3

• K2CO3 + Zn(NO3)2 → ZnCO3 + 2KNO3

• Zn^2+ + CO3^2- → ZnCO3

• 2K+ + CO3^2- → ZnCO3