Net Ionic Equations and Solubility

This video tutorial explains how to write net ionic equations, starting with predicting products in a double replacement reaction. It covers balancing molecular equations and converting them into total and net ionic equations by identifying and removing spectator ions. The tutorial includes examples with sodium iodide and lead nitrate, as well as potassium phosphate and magnesium chloride, emphasizing solubility rules and the crisscross method for determining compound formulas.

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

• Identifying spectator ions

• Predicting the products

• Writing the molecular equation

• Balancing the equation

Which of the following compounds is always soluble?

• Lead iodide

• Sodium nitrate

• Silver chloride

• Mercury bromide

What is the charge of the lead ion in lead nitrate?

• +1

• +2

• +3

• +4

What is the purpose of balancing a molecular equation?

• To determine solubility

• To predict the products

• To ensure mass conservation

• To identify spectator ions

Which ions are considered spectator ions in the reaction between sodium iodide and lead nitrate?

• Sodium and iodide ions

• Lead and nitrate ions

• Lead and iodide ions

• Sodium and nitrate ions

What is the net ionic equation?

• The equation predicting products

• The equation after removing spectator ions

• The equation showing all ions

• The balanced molecular equation

In the second example, what is the charge of the phosphate ion?

• -3

• -4

• -2

• -1

What is the solubility of magnesium phosphate?

• Depends on temperature

• Insoluble

• Partially soluble

• Soluble

How many potassium ions are present in the balanced equation for the reaction between potassium phosphate and magnesium chloride?

• 8

• 4

• 2

• 6

What type of reaction occurs when a solid forms from two aqueous solutions?

• Decomposition reaction

• Redox reaction

• Synthesis reaction

• Precipitation reaction