Solubility and Equilibrium Concepts

The video tutorial explains the common ion effect on solubility equilibrium using lead(II) chloride as an example. It describes how adding a common ion, such as chloride from potassium chloride, disrupts equilibrium, causing a shift according to Le Chatelier's principle. This shift results in decreased solubility of the salt. The tutorial also covers the reaction quotient and Ksp, and demonstrates calculating molar solubility with and without a common ion using an ICE table.

What is the mole ratio of Pb2+ to Cl- ions in a saturated solution of lead(II) chloride?

• 1:2

• 2:2

• 1:1

• 2:1

What happens to the equilibrium when potassium chloride is added to the solution?

• The concentration of Pb2+ increases.

• The system is no longer at equilibrium.

• The system shifts to the right.

• The system remains at equilibrium.

According to Le Chatelier's principle, how does the system respond to an increase in chloride ions?

• The system shifts to the right.

• The system shifts to the left.

• The system remains unchanged.

• The concentration of K+ increases.

What is the common ion in the example of lead(II) chloride and potassium chloride?

• Cl-

• PbCl2

• K+

• Pb2+

How does the presence of a common ion affect the solubility of a slightly soluble salt?

• Doubles the solubility

• Has no effect

• Decreases solubility

• Increases solubility

What happens to the reaction quotient (Q) when chloride ions are added to the solution?

• Q becomes less than Ksp

• Q becomes equal to Ksp

• Q becomes greater than Ksp

• Q does not change

What is the effect of a shift to the left on the amount of PbCl2?

• Decreases the amount of PbCl2

• Increases the amount of PbCl2

• No change in PbCl2

• Dissolves all PbCl2

What is the purpose of using an ICE table in solubility calculations?

• To find the volume of the solution

• To determine equilibrium concentrations

• To calculate initial concentrations

• To measure temperature changes

How does the molar solubility of lead(II) chloride change in the presence of a common ion?

• It doubles

• It remains the same

• It increases by a factor of 10

• It decreases by a factor of 10

What is the approximate molar solubility of lead(II) chloride without a common ion?

• 0.17 M

• 0.10 M

• 0.016 M

• 0.0017 M