Solubility and Common Ion Effects

The video tutorial explains the principles of equilibrium and solubility, focusing on the molar solubility of magnesium fluoride. It discusses the common ion effect and its impact on solubility, providing a detailed calculation of solubility with and without the presence of a common ion. The tutorial concludes with real-world implications of solubility in various contexts.

What principle helps us understand how equilibrium shifts when a system is disturbed?

• Le Chatelier's Principle

• Boyle's Law

• Avogadro's Law

• Dalton's Law

What does molar solubility specifically refer to?

• The number of moles of solute that dissolve in one liter of solution

• The number of moles of solute in a mole of solution

• The number of moles of solute in a liter of solvent

• The number of moles of solute in a kilogram of solvent

In the solubility product expression for magnesium fluoride, what is the exponent of the fluoride ion concentration?

• 3

• 1

• 4

• 2

What effect describes the decreased solubility of a salt when one of its ions is already present in the solution?

• Precipitation Effect

• Common Ion Effect

• Dissolution Effect

• Ionization Effect

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

• Increases solubility

• Decreases solubility

• Has no effect

• Doubles the solubility

Why are approximations useful in solving solubility problems with common ions?

• They are not useful at all

• They are only used for theoretical purposes

• They provide exact solutions

• They simplify complex calculations

What is the approximate molar solubility of magnesium fluoride in pure water?

• 2.65 moles per liter

• 7.4 x 10^-9 moles per liter

• 2.65 x 10^-4 moles per liter

• 0.1 moles per liter

What happens to the solubility of magnesium fluoride when sodium fluoride is added to the solution?

• It increases significantly

• It doubles

• It decreases significantly

• It remains unchanged

In the context of solubility, what does a small Ksp value indicate?

• No solubility

• Low solubility

• High solubility

• Infinite solubility

Why might a substance that is soluble in pure water precipitate in a biological system?

• Due to the absence of light

• Due to the presence of other dissolved substances

• Because of a decrease in temperature

• Because of an increase in pressure