The video tutorial explains how to write a balanced net ionic equation for the reaction between zinc chloride (ZnCl2) and potassium hydroxide (KOH). It begins by balancing the molecular equation and then discusses the solubility rules to determine the states of the substances involved. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into their ions. Finally, it derives the net ionic equation by removing spectator ions and ensuring the equation is balanced in terms of charge and atoms.

What is the first step in balancing the molecular equation for ZnCl2 and KOH?

• Add a coefficient of 2 in front of ZnCl2

• Add a coefficient of 1 in front of Zn(OH)2

• Add a coefficient of 2 in front of KOH

• Add a coefficient of 3 in front of KCl

According to solubility rules, which of the following is generally soluble in water?

• Zinc hydroxide

• Iron(III) hydroxide

• Potassium hydroxide

• Calcium hydroxide

What is the state of zinc hydroxide in the reaction?

• Aqueous

• Gas

• Solid

• Liquid

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

• 3+

• 2+

• 0

• 1+

In the complete ionic equation, how many chloride ions are present?

• Four

• Three

• Two

• One

What is the purpose of identifying spectator ions in a reaction?

• To determine the reaction rate

• To simplify the net ionic equation

• To identify the limiting reactant

• To balance the equation

Which ions are considered spectator ions in this reaction?

• Oxygen ions

• Zinc ions

• Hydroxide ions

• Potassium ions

What is the net ionic equation for the reaction between ZnCl2 and KOH?

• 2K^+ + 2OH^- → 2KOH

• Zn^2+ + 2Cl^- → ZnCl2

• Zn^2+ + 2K^+ → ZnK2

• Zn^2+ + 2OH^- → Zn(OH)2

How is charge conservation demonstrated in the net ionic equation?

• By having more negative ions than positive ions

• By having equal numbers of positive and negative charges

• By having more positive ions than negative ions

• By having no ions present

What ensures that the net ionic equation is balanced?

• Equal number of electrons on each side

• Equal number of compounds on each side

• Equal number of atoms and charges on each side

• Equal number of molecules on each side