Calcium Hydroxide and Ionic Equations

The video tutorial explains how to balance net ionic equations, focusing on the reaction between calcium and water. It covers writing balanced molecular equations, determining the states of compounds using a solubility table, and understanding net ionic equations. The tutorial also explores an alternative approach by treating compounds as strong electrolytes, even if not fully appropriate. The video concludes with a demonstration of rewriting equations by dissociating ions.

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

• Calculate the molar mass of reactants

• Identify the spectator ions

• Write the balanced molecular equation

• Determine the solubility of the reactants

What is the state of calcium when it is by itself in the reaction?

• Liquid

• Gas

• Solid

• Aqueous

How do you determine if calcium hydroxide is soluble?

• By checking a solubility table

• By measuring its pH

• By observing its color change

• By calculating its molar mass

What does 'ss' indicate on a solubility table?

• Slightly soluble

• Strongly soluble

• Not soluble

• Super soluble

Why don't we split solids, liquids, and gases in net ionic equations?

• They are not reactive

• They are spectator ions

• They are always soluble

• They do not dissociate into ions

What is the charge of the calcium ion when it dissociates?

• 2+

• 2-

• 1-

• 1+

What is the charge of the hydroxide ion?

• 2-

• 1-

• 2+

• 1+

What happens to the state of calcium hydroxide if it is assumed to be a strong electrolyte?

• It becomes a liquid

• It becomes aqueous

• It becomes a gas

• It remains a solid

What is the net ionic equation if calcium hydroxide is considered a strong electrolyte?

• Ca(s) + H2O(l) → Ca(OH)2(aq) + H2(g)

• Ca(s) + 2H2O(l) → Ca2+(aq) + 2OH-(aq) + H2(g)

• Ca(s) + 2H2O(l) → Ca(OH)2(s) + H2(g)

• Ca2+(aq) + 2OH-(aq) → Ca(OH)2(s)

Why can't we cross out any spectator ions in the net ionic equation?

• All ions are the same on both sides

• There are no ions present

• There are no common ions on both sides

• The reaction is not balanced