Balancing Ionic Equations and Electrolytes

This video tutorial explains how to write a balanced net ionic equation for the reaction between iron(III) chloride and calcium hydroxide. It covers balancing the molecular equation, determining the states of substances using solubility rules, and splitting strong electrolytes into ions for the complete ionic equation. The tutorial also identifies and removes spectator ions to derive the net ionic equation, ensuring that both atoms and charges are balanced. The final step involves reducing coefficients to simplify the equation.

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

• Identify the spectator ions

• Balance the molecular equation

• Determine the states of the reactants

• Write the complete ionic equation

How many chloride ions are present after balancing the molecular equation?

• Four

• Two

• Eight

• Six

Which of the following is considered a strong electrolyte in the reaction?

• Calcium hydroxide

• Iron(III) chloride

• Iron(III) hydroxide

• Water

What is the state of iron(III) hydroxide in the reaction?

• Solid

• Gas

• Liquid

• Aqueous

What is the charge on the calcium ion in the complete ionic equation?

• 1+

• 2+

• 3+

• 0

Which ions are considered spectator ions in this reaction?

• Iron(III) ions

• Calcium ions

• Hydroxide ions

• Chloride ions

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

• Positive

• Negative

• Zero

• Undefined

What should be done to the coefficients in the net ionic equation to simplify it?

• Divide by two

• Subtract one

• Add one

• Multiply by two

What is the final balanced net ionic equation for the reaction?

• 2Fe^3+ + 6Cl^- -> 2FeCl3

• Fe^3+ + 3OH^- -> Fe(OH)3

• 2Fe^3+ + 6OH^- -> 2Fe(OH)3

• Fe(OH)3 + 3Ca^2+ -> 3Ca^2+ + 2Fe^3+

Why is it important to remove spectator ions when writing a net ionic equation?

• To simplify the equation

• To balance the equation

• To identify the precipitate

• To determine the reaction rate