Solubility and Common Ion Effects

The video tutorial covers factors affecting the solubility of insoluble salts, focusing on the common ion effect. It explains how adding a common ion, like sodium fluoride, shifts equilibrium and decreases solubility. The tutorial emphasizes using ICE tables for solving common ion problems and demonstrates calculating molar solubility of calcium fluoride in pure water and with added sodium fluoride. The key takeaway is that adding a common ion reduces solubility by shifting equilibrium towards the solid form.

What is the primary focus of the last section of chapter 15?

• Factors affecting the solubility of insoluble salts

• The role of temperature in solubility

• The effect of pH on solubility

• The impact of pressure on solubility

What happens to the equilibrium when a common ion is added to a solution?

• Equilibrium shifts to the left

• Equilibrium remains unchanged

• Equilibrium shifts to the right

• Equilibrium is destroyed

How does adding a common ion affect the solubility of an insoluble salt?

• Increases solubility

• Decreases solubility

• Has no effect on solubility

• Doubles the solubility

Why is using an ICE table recommended when dealing with common ion problems?

• It simplifies the math

• It is required by all chemistry textbooks

• It is the only method to solve these problems

• It helps track changes in concentration

What is the molar solubility of calcium fluoride in pure water?

• 1.0 times 10 to the minus 3 molar

• 3.4 times 10 to the minus 11 molar

• 4.0 times 10 to the minus 5 molar

• 2.0 times 10 to the minus 4 molar

What is the Ksp value used in the calculation of calcium fluoride's solubility?

• 3.4 times 10 to the minus 11

• 2.0 times 10 to the minus 4

• 1.0 times 10 to the minus 3

• 4.0 times 10 to the minus 5

What is the initial concentration of fluoride when sodium fluoride is added?

• 0.015

• 0.005

• 0.020

• 0.010

What assumption is made to simplify the math when K is less than 10 to the minus 3?

• x is squared

• x can be ignored

• x is doubled

• x is halved

What is the final x value when calculating solubility with a common ion?

• 4.0 times 10 to the minus 5 molar

• 1.0 times 10 to the minus 3 molar

• 2.0 times 10 to the minus 4 molar

• 3.4 times 10 to the minus 7 molar

How does the solubility change when a common ion is added compared to without it?

• It increases

• It doubles

• It decreases

• It remains the same