Balancing Ionic Reactions and Solubility

The video tutorial explains how to write a balanced net ionic equation for the reaction between magnesium nitrate (Mg(NO3)2) and potassium hydroxide (KOH). It begins by balancing the molecular equation, then discusses the solubility and states of the reactants and products. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into their ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring the charge balance and summarizing the balanced net ionic equation.

What is the first step in balancing the molecular equation for the reaction between magnesium nitrate and potassium hydroxide?

• Balance the potassium ions

• Balance the nitrate ions

• Balance the magnesium ions

• Balance the hydroxide ions

Which of the following is true about the solubility of magnesium nitrate?

• It does not dissociate

• It is very soluble

• It is slightly soluble

• It is insoluble in water

What is the state of magnesium hydroxide in the reaction?

• Gas

• Solid

• Aqueous

• Liquid

When forming the complete ionic equation, what charge does the magnesium ion have?

• 2-

• 1+

• 2+

• 1-

Which ions are considered spectator ions in this reaction?

• Magnesium and potassium ions

• Nitrate and hydroxide ions

• Potassium and nitrate ions

• Magnesium and hydroxide ions

What is the net ionic equation for the reaction between magnesium nitrate and potassium hydroxide?

• Mg^2+ + 2OH^- → Mg(OH)2

• 2K^+ + 2NO3^- → 2KNO3

• Mg^2+ + 2NO3^- → Mg(NO3)2

• 2K^+ + 2OH^- → 2KOH

Why do we not split solids in net ionic equations?

• They are already balanced

• They are spectator ions

• They do not dissociate in water

• They are not reactive

What is the net charge on both sides of the net ionic equation?

• 0

• 2-

• 2+

• 1+

How do you ensure the net ionic equation is balanced?

• By balancing both charges and atoms

• By balancing the coefficients only

• By balancing the atoms only

• By balancing the charges only

What happens to the precipitate formed in the reaction?

• It dissolves in water

• It remains in solution

• It falls to the bottom of the test tube

• It reacts with other ions