This video tutorial explains how to write a balanced net ionic equation for the reaction between phosphoric acid (H3PO4) and potassium hydroxide (KOH). It begins with balancing the molecular equation, followed by determining the states of each substance. The tutorial then demonstrates how to form the complete ionic equation by splitting strong electrolytes into ions. Finally, it shows how to derive the net ionic equation by removing spectator ions, ensuring the conservation of atoms and charge.

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

• Split strong electrolytes into ions

• Determine the states of substances

• Balance the molecular equation

• Identify spectator ions

How many potassium ions are needed to balance the molecular equation for H3PO4 and KOH?

• One

• Four

• Two

• Three

What is the state of phosphoric acid in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

Which of the following is a strong electrolyte?

• Phosphoric acid

• Water

• Potassium phosphate

• Potassium hydroxide

What is the charge of the hydroxide ion?

• 1+

• 1-

• 2-

• 2+

Why don't we split liquids into ions in the complete ionic equation?

• They are already balanced

• They do not dissociate

• They are spectator ions

• They are weak electrolytes

What is the purpose of identifying spectator ions?

• To balance the equation

• To identify strong electrolytes

• To simplify the net ionic equation

• To determine the states of substances

Which ions are considered spectator ions in this reaction?

• Hydroxide ions

• Potassium ions

• Phosphate ions

• Hydrogen ions

What is conserved in a net ionic equation?

• Both mass and charge

• Only charge

• Only mass

• Neither mass nor charge

What is the net ionic equation for the reaction between phosphoric acid and potassium hydroxide?

• H3PO4 + 3KOH → 3K+ + PO4^3- + 3H2O

• H3PO4 + KOH → K3PO4 + H2O

• H3PO4 + 3OH- → PO4^3- + 3H2O

• 3K+ + PO4^3- → K3PO4