Solubility Rules and Ionic Equations

The video tutorial explains how to write net ionic equations using sodium sulfate (Na2SO4) and potassium nitrate (KNO3) as examples. It begins by balancing the molecular equation, ensuring the number of atoms for each element is equal on both sides. The tutorial then discusses the solubility of compounds containing sodium and potassium, noting that they dissolve and dissociate into ions in water. Since both reactants and products are soluble and dissociate into ions, no net ionic equation is formed, as no reaction occurs. The video concludes by reiterating that no chemical change takes place.

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

• Balance the molecular equation

• Write the ionic equation

• Identify the spectator ions

• Determine the solubility of compounds

How many sodium atoms are needed on each side of the balanced molecular equation?

• One

• Two

• Three

• Four

What happens to compounds containing sodium when dissolved in water?

• They react with water

• They dissolve and dissociate into ions

• They remain undissolved

• They form a precipitate

What is the role of potassium in the reaction?

• It reacts with sodium

• It dissolves and dissociates into ions

• It remains as a solid

• It forms a precipitate

Which of the following is true about the solubility of compounds with potassium?

• They react with water

• They are usually soluble

• They are usually insoluble

• They form a gas

Why is there no net ionic equation for the reaction between sodium sulfate and potassium nitrate?

• Because a precipitate forms

• Because all compounds are insoluble

• Because the reaction is incomplete

• Because all compounds dissolve and dissociate into ions

What is the result when sodium sulfate and potassium nitrate are mixed in water?

• A chemical reaction occurs

• A gas is released

• A precipitate forms

• No reaction occurs

What is the significance of the solubility rules in this reaction?

• They show the reaction rate

• They determine the color of the solution

• They indicate that no reaction occurs

• They help predict the formation of a precipitate