Chemical Reactions and Ionic Compounds

The video tutorial explains how to write a net ionic equation for the reaction between calcium nitrate and potassium phosphate. It covers balancing the molecular equation, determining the solubility states of the compounds, splitting strong electrolytes into ions, and forming the complete ionic equation. The tutorial concludes with deriving the net ionic equation by removing spectator ions, resulting in the formation of a solid precipitate, calcium phosphate.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the net ionic equation directly

Which of the following is true about nitrates in aqueous solutions?

• They do not dissociate into ions

• They are generally insoluble

• They form a solid precipitate

• They are very soluble

What does the 's' symbol indicate in a solubility table?

• The compound is insoluble

• The compound is soluble

• The compound is a gas

• The compound is a liquid

What charge does a calcium ion typically have?

• 1+

• 2+

• 3+

• 1-

How many nitrate ions are present when calcium nitrate dissociates?

• Eight

• Six

• Four

• Two

What is the charge of a phosphate ion?

• 3-

• 4-

• 2-

• 1-

What is a spectator ion?

• An ion that participates in the reaction

• An ion that remains unchanged on both sides of the equation

• An ion that forms a precipitate

• An ion that changes state during the reaction

Which ions are crossed out in the complete ionic equation?

• Spectator ions

• Ions that form a solid

• Ions that are gases

• Ions that are soluble

What is formed when calcium ions react with phosphate ions?

• Calcium nitrate

• Potassium phosphate

• Calcium phosphate

• Potassium nitrate

What is the final product of the reaction between calcium nitrate and potassium phosphate?

• Gas

• Solid precipitate

• Aqueous solution

• Liquid