Net Ionic Equations and Solubility

The video tutorial explains how to write and balance net ionic equations, using the reaction between chromium(III) nitrate and sodium phosphate as an example. It covers balancing the molecular equation, determining the states of substances based on solubility rules, and creating complete and net ionic equations. Spectator ions are identified and removed to finalize the net ionic equation, ensuring charge and atom balance.

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

• Determine the states of substances

• Identify spectator ions

• Split strong electrolytes into ions

• Balance the molecular equation

Why is sodium phosphate considered soluble?

• Because phosphates are always soluble

• Because it is a group one element compound

• Because it contains chromium

• Because it forms a precipitate

What is the state of chromium phosphate in the reaction?

• Aqueous

• Liquid

• Gas

• Solid

What do you do with strong electrolytes in the complete ionic equation?

• Leave them as molecules

• Split them into ions

• Convert them to solids

• Ignore them

Which ions are considered spectator ions in this reaction?

• Chromium ions

• Phosphate ions

• Sodium and nitrate ions

• All ions are spectator ions

What is the purpose of removing spectator ions?

• To determine solubility

• To identify the precipitate

• To balance the charge

• To simplify the equation

How do you ensure the net ionic equation is balanced?

• By ensuring the charges are balanced

• By adding more reactants

• By removing all ions

• By checking the number of atoms only

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

• Variable

• Zero

• Negative

• Positive

What is the role of Dr. B in the video?

• To demonstrate a chemical experiment

• To introduce new chemical elements

• To explain the balanced net ionic equation

• To discuss the history of chemistry

What is the final product of the reaction between chromium(III) nitrate and sodium phosphate?

• Solid chromium phosphate

• Solid sodium phosphate

• Aqueous sodium nitrate

• Aqueous chromium nitrate