Net Ionic Equations and Reactions

This video tutorial explains how to write the balanced net ionic equation for the reaction between strontium nitrate and magnesium sulfate. It begins with balancing the molecular equation, then discusses the solubility of the reactants and products to determine their states. The tutorial proceeds to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring charge conservation and atom balance in the final equation.

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

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

• Identify the spectator ions

Why are nitrates considered very soluble?

• They dissociate completely in water

• They are insoluble in water

• They form strong covalent bonds

• They are always in gaseous state

What is the state of strontium sulfate in the reaction?

• Liquid

• Gaseous

• Solid

• Aqueous

What charge does the strontium ion have in the complete ionic equation?

• 2-

• 1-

• 2+

• 1+

Which ion is not split in the net ionic equation?

• Strontium sulfate

• Sulfate ion

• Nitrate ion

• Magnesium ion

What is the role of spectator ions in a reaction?

• They form the precipitate

• They participate in the reaction

• They change the state of the reaction

• They remain unchanged and are not part of the net ionic equation

What is the net charge of the balanced net ionic equation?

• 1+

• 0

• 2+

• 2-

Why is it important to ensure that the atoms are balanced in the net ionic equation?

• To conserve mass

• To change the reaction rate

• To alter the solubility

• To increase the temperature

What is the final product formed in the reaction between strontium nitrate and magnesium sulfate?

• Strontium sulfate

• Strontium nitrate

• Magnesium nitrate

• Magnesium sulfate

What does the 's' symbol indicate in the context of the reaction?

• Solution

• Sublimation

• Soluble

• Solid