Net Ionic Equations and Balancing

This video tutorial explains how to write and balance the net ionic equation for the reaction between sodium phosphate (Na3PO4) and cobalt(II) chloride (CoCl2). It covers balancing the molecular equation, determining the states of compounds, forming the complete ionic equation, and deriving the net ionic equation by removing spectator ions. The tutorial emphasizes the importance of balancing charges and ensuring the equation is neutral.

What is the first step in balancing the molecular equation for sodium phosphate and cobalt(II) chloride?

• Balance the cobalt ions.

• Balance the phosphate ions.

• Balance the chloride ions.

• Balance the sodium atoms.

Why is sodium phosphate considered soluble in water?

• Because it is a chloride compound.

• Because it contains cobalt, which is always soluble.

• Because it contains sodium, which is always soluble.

• Because all phosphates are soluble.

What is the state of cobalt phosphate in the reaction?

• Gas

• Aqueous

• Liquid

• Solid

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

• Two

• Four

• Six

• Three

What charge does the phosphate ion carry in the complete ionic equation?

• 1-

• 2-

• 4-

• 3-

Which ions are considered spectator ions in this reaction?

• Sodium and chloride ions

• Phosphate and cobalt ions

• Cobalt and chloride ions

• Sodium and phosphate ions

What is the net ionic equation for the reaction between sodium phosphate and cobalt(II) chloride?

• 3 Co^2+ + 2 PO4^3- → Co3(PO4)2

• 6 Na+ + 6 Cl- → 6 NaCl

• Na3PO4 + CoCl2 → NaCl + Co3(PO4)2

• 2 Na+ + 2 Cl- → 2 NaCl

Why is it important to ensure the charges are balanced in the net ionic equation?

• To ensure the equation is neutral.

• To make the equation more complex.

• To increase the number of spectator ions.

• To simplify the equation.

What is the total charge on the reactant side of the net ionic equation?

• 6-

• 0

• 3+

• 6+

In the final net ionic equation, which ions are written first?

• Spectator ions

• Neutral molecules

• Positive ions

• Negative ions