Net Ionic Equations and Spectator Ions

The video tutorial explains how to write the net ionic equation for the reaction between hydrobromic acid (HBr) and potassium hydrogen carbonate (KHCO3). It begins by balancing the molecular equation and determining the states of each compound. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and crossed out to derive the net ionic equation. The final net ionic equation is balanced in terms of both atoms and charge, ensuring a net charge of zero.

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

• Balance the molecular equation

• Identify spectator ions

• Determine the states of substances

• Split strong electrolytes into ions

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

• HBr

• CO2

• H2O

• KHCO3

What state is assigned to potassium hydrogen carbonate in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

What is the charge of the hydrogen ion in the complete ionic equation?

• 0

• +1

• +2

• -1

Which ion is not split in the net ionic equation?

• Bromide ion

• Carbon dioxide

• Hydrogen ion

• Potassium ion

What is the role of spectator ions in a chemical reaction?

• They participate in the reaction

• They balance the equation

• They change the state of the reaction

• They remain unchanged and do not participate

Which ions are considered spectator ions in this reaction?

• Hydrogen and bromide ions

• Hydrogen and potassium ions

• Potassium and bromide ions

• Carbon dioxide and water

What must be balanced in a net ionic equation?

• Neither mass nor charge

• Only the charge

• Both mass and charge

• Only the mass

What is the net charge of the products in the balanced net ionic equation?

• +1

• -1

• 0

• +2

What is the final product of the reaction between HBr and KHCO3?

• CO2 and KBr

• H2O and KBr

• KBr and H2O

• H2O and CO2