Net Ionic Equations and Electrolytes

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between hydrogen cyanide (HCN) and sodium hydroxide (NaOH). It begins with balancing the molecular equation and identifying the states of each substance. The tutorial explains the difference between strong and weak electrolytes, emphasizing the importance of splitting strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. Finally, the video ensures that both charge and mass are balanced in the final equation.

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 true about HCN in water?

• It is a strong acid

• It is a weak acid

• It dissociates completely

• It is insoluble

What is the state of sodium hydroxide in water?

• Solid

• Gas

• Liquid

• Aqueous

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

• It is a gas

• It is a strong electrolyte

• It is a weak electrolyte

• It is insoluble

What charge does the sodium ion have?

• 2-

• 1-

• 1+

• 2+

Which ion is considered a spectator ion in this reaction?

• Sodium ion

• Cyanide ion

• Hydrogen ion

• Hydroxide ion

What is the purpose of removing spectator ions?

• To simplify the net ionic equation

• To determine solubility

• To balance the equation

• To identify strong acids

What must be balanced in the final net ionic equation?

• Only the charge

• Only the mass

• Both charge and mass

• Neither charge nor mass

What is the charge on the cyanide ion?

• 2+

• 1+

• 1-

• 2-

What is the final product in the net ionic equation for HCN and NaOH?

• NaOH

• NaCN

• HCN

• H2O