Net Ionic Equations and Solubility

The video tutorial explains how to balance net ionic equations, starting with balancing the molecular equation for chromium-3 chloride and silver nitrate. It covers writing the states of substances, identifying precipitates, and forming complete and net ionic equations. The tutorial emphasizes the importance of charge conservation and atom balance in the final net ionic equation.

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

• Identify spectator ions

• Split strong electrolytes into ions

• Write the states of each substance

• Balance the molecular equation

How many chlorine atoms are needed to balance the molecular equation for CrCl3 and AgNO3?

• 3

• 2

• 1

• 4

Which of the following is generally soluble in water?

• Calcium carbonate

• Silver chloride

• Nitrates

• Lead sulfate

What is the state of silver chloride in the reaction?

• Liquid

• Gas

• Solid

• Aqueous

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

• Ignore them

• Convert them to solids

• Split them into ions

• Leave them as compounds

Which ions are considered spectator ions in this reaction?

• Nitrate ions

• Chloride ions

• Silver ions

• Chromium ions

What is the net charge of the reactants and products in the net ionic equation?

• Negative

• Positive

• Zero

• Variable

Why is it important to ensure the net charge is zero in the net ionic equation?

• To conserve mass

• To simplify the equation

• To balance the equation

• To conserve charge

What happens to the coefficients in the final net ionic equation?

• They are doubled

• They are reduced to one

• They remain unchanged

• They are eliminated

What is the purpose of balancing net ionic equations?

• To determine solubility

• To identify precipitates

• To ensure mass and charge conservation

• To predict reaction speed