Net Ionic Equations and Strong Acids

This video tutorial explains how to write a balanced net ionic equation for the reaction between hydrobromic acid (HBr) and sodium hydroxide (NaOH). It begins with balancing the molecular equation and identifying the states of each substance. The tutorial then demonstrates how to split strong electrolytes into their ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by emphasizing the conservation of charge and mass in the reaction.

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

• Split strong electrolytes into ions

• Write the states of substances

• Balance the molecular equation

• Identify spectator ions

Which of the following is a strong acid that dissociates completely in water?

• HCl

• H2SO4

• HBr

• HF

What state symbol is used for substances that dissociate completely in water?

• s

• l

• g

• aq

What is the charge of the hydroxide ion?

• 1+

• 1-

• 2+

• 2-

In the complete ionic equation, which ions are not split apart?

• Bromide ions

• Water molecules

• Sodium ions

• Hydrogen ions

What are spectator ions?

• Ions that form a precipitate

• Ions that are gases

• Ions that do not change during the reaction

• Ions that participate in the reaction

Which ions are crossed out in the net ionic equation for HBr and NaOH?

• Water molecules

• Sodium and bromide ions

• Hydrogen and hydroxide ions

• All ions

What is conserved in a balanced net ionic equation?

• Neither mass nor charge

• Only charge

• Both mass and charge

• Only mass

How many hydrogen atoms are present on each side of the balanced net ionic equation for HBr and NaOH?

• One

• Two

• Four

• Three

What is the final product of the reaction between HBr and NaOH in the net ionic equation?

• NaBr

• H2O

• NaOH

• HBr