Net Ionic Equations and Solubility

The video tutorial explains how to write balanced net ionic equations, starting with balancing the molecular equation for magnesium nitrate and sodium chromate. It discusses the process of writing complete ionic equations by identifying spectator ions and determining the states of substances. The tutorial highlights the importance of recognizing when a substance forms a precipitate, which affects the net ionic equation. The video concludes with a demonstration of how to handle solids in net ionic equations.

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

• Write the complete ionic equation

• Balance the molecular equation

• Identify spectator ions

• Determine the solubility of compounds

How do you balance the molecular equation for magnesium nitrate and sodium chromate?

• Add water molecules

• Adjust the coefficients of the compounds

• Change the subscripts of the ions

• Remove spectator ions

What does it mean when all substances in a reaction are aqueous?

• They form a solid precipitate

• They react with each other

• They do not dissolve in water

• They dissolve and split into ions

What is the purpose of writing the complete ionic equation?

• To show all ions present in the reaction

• To determine the reaction rate

• To balance the molecular equation

• To identify the products

What are spectator ions?

• Ions that do not change during the reaction

• Ions that form a precipitate

• Ions that are insoluble

• Ions that participate in the reaction

What happens when all ions are crossed out in a net ionic equation?

• A gas is released

• A precipitate forms

• No reaction occurs

• A new compound is formed

How does the solubility of MgCrO4 affect the net ionic equation?

• It affects whether a reaction occurs

• It alters the pH of the solution

• It determines the color of the solution

• It changes the temperature of the reaction

What is the result if MgCrO4 is considered insoluble?

• It dissolves completely

• It forms a gas

• It remains in solution

• It forms a solid precipitate

Why might a teacher consider MgCrO4 as a solid?

• Because it is a liquid

• Because it is a gas

• Because it is insoluble or slightly soluble

• Because it is highly reactive

What should you do if your teacher says MgCrO4 is a solid?

• Treat it as aqueous

• Ignore the teacher's instruction

• Write it as a solid in the net ionic equation

• Consider it as a gas