Ionic and Aqueous Solutions Concepts

This video tutorial explains how to write the equation for sodium sulfate (Na2SO4) plus water (H2O). It covers the ionic nature of sodium sulfate, identifying sodium as a metal and sulfate as a polyatomic ion. The video discusses the ionic charges of sodium and sulfate, and how sodium sulfate dissociates into its ions when dissolved in water, forming an aqueous solution. The tutorial concludes with a summary of the dissolution process and the resulting equation.

What type of ion is sulfate (SO4) considered to be?

• Polyatomic ion

• Cation

• Anion

• Monatomic ion

What is the ionic charge of sodium (Na) when it forms an ion?

• -1

• +2

• 0

• +1

How is the charge of the sulfate ion (SO4) determined?

• By its color

• By looking at the periodic table

• By measuring its mass

• By using a table of common polyatomic ions

What happens to sodium sulfate when it is added to water?

• It evaporates

• It remains unchanged

• It dissociates into ions

• It forms a precipitate

What ions are formed when sodium sulfate dissociates in water?

• Na- and SO4+

• Na2+ and SO4-

• Na+ and SO4 2-

• Na+ and Cl-

What does the term 'aqueous' mean in the context of this reaction?

• Dissolved in water

• Gaseous state

• Evaporated

• Solid state

Why is it unnecessary to write H2O on the product side of the equation?

• Because it is a solid

• Because it is a gas

• Because it is already represented as aqueous

• Because it is not involved in the reaction