Weak Acids and Net Ionic Equations

This video tutorial explains how to write a balanced net ionic equation for the reaction between hypochlorous acid (HClO) and sodium hydroxide (NaOH). It begins by ensuring the molecular equation is balanced and then identifies the states of each substance. HClO is identified as a weak acid, while NaOH is a strong base. The video demonstrates how to split strong electrolytes into ions to form a complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The tutorial concludes by verifying the conservation of charge and mass.

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

• Balance the molecular equation

• Identify spectator ions

• Split strong electrolytes into ions

• Determine the states of substances

Why is HClO considered a weak acid?

• It fully dissociates in water

• It is not listed among common strong acids

• It is a strong electrolyte

• It reacts violently with bases

What is the state of NaOH in the reaction?

• Aqueous

• Liquid

• Gas

• Solid

Which of the following is a strong electrolyte?

• HClO

• NaOH

• CLO-

• H2O

What is the purpose of identifying spectator ions?

• To determine the reaction rate

• To simplify the net ionic equation

• To balance the equation

• To identify the products

Which ion is a spectator ion in this reaction?

• H+

• Na+

• CLO-

• OH-

What is conserved in a balanced net ionic equation?

• Only charge

• Neither mass nor charge

• Only mass

• Both mass and charge

What happens to water in the net ionic equation?

• It is split into ions

• It remains as a liquid

• It reacts with NaOH

• It is a spectator ion

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

• Variable

• Neutral

• Negative

• Positive

What is the final product of the reaction between HClO and NaOH?

• NaCl

• HCl

• H2O

• NaClO