Molar Solubility and Common Ion Effect

The video tutorial covers the common ion effect, explaining how the presence of a common ion in a solution affects the solubility of a salt. It uses examples of zinc hydroxide and calcium hydroxide to demonstrate the application of Le Chatelier's principle and the solubility product constant. The tutorial also includes a mathematical approach to calculating molar solubility and provides a step-by-step guide to solving solubility problems using ICE tables and approximation methods.

What is the common ion effect primarily concerned with?

• Increasing the solubility of salts

• Decreasing the solubility of salts

• Changing the color of solutions

• Increasing the temperature of solutions

Which principle is applied in common ion problems to predict the shift in equilibrium?

• Dalton's Law

• Avogadro's Law

• Le Chatelier's Principle

• Boyle's Law

In the context of zinc hydroxide, what happens when a common ion is added to the solution?

• The solution becomes basic

• The solubility of zinc hydroxide increases

• The solubility of zinc hydroxide decreases

• The solution becomes acidic

What is the purpose of setting up an ICE table in solubility problems?

• To calculate the temperature change

• To determine the initial, change, and equilibrium concentrations

• To measure the pH of the solution

• To find the boiling point of the solution

What assumption is made in the assumption-based method for calculating molar solubility?

• The concentration of the common ion is negligible

• The temperature remains constant

• The change in concentration is negligible

• The change in concentration is significant

In the calcium hydroxide example, what is the initial concentration of the calcium ion?

• 0.3 M

• 0.1 M

• 0.2 M

• 0.4 M

What is the solubility product constant (Ksp) used for in solubility calculations?

• To determine the color of the solution

• To calculate the boiling point

• To find the equilibrium concentrations of ions

• To measure the pH

In the silver chloride example, what is the initial concentration of sodium chloride?

• 0.003 M

• 0.002 M

• 0.001 M

• 0.004 M

What is the solubility product constant (Ksp) for silver chloride?

• 1.8 x 10^-10

• 1.8 x 10^-8

• 1.8 x 10^-7

• 1.8 x 10^-6

What is the final molar solubility of silver chloride in the sodium chloride solution?

• 1.8 x 10^-8

• 1.8 x 10^-7

• 1.8 x 10^-6

• 1.8 x 10^-5