More Aspects Of Aqueous Equilibrium

Question 1

What is the definition of aqueous equilibrium?

Answer 1

A state in which the rate of dissolution of a solute is equal to the rate of precipitation of the solute.

Question 2

True or False: Aqueous equilibrium occurs when a solute completely dissolves in a solvent.

Answer 2

False

Question 3

What is the equation for the solubility product constant (Ksp)?

Answer 3

Ksp = [A]^a[B]^b, where A and B are the ions in a sparingly soluble salt and a, b are the stoichiometric coefficients

Question 4

In a saturated solution, what is happening at the molecular level?

Answer 4

There is a dynamic equilibrium between the dissolved ions and the solid salt

Question 5

What is the common ion effect?

Answer 5

The decrease in the solubility of a sparingly soluble salt when a common ion is added to the solution

Question 6

What is the effect of temperature on the solubility of most solid solutes in water?

Answer 6

Solubility typically increases with temperature

Question 7

Fill in the blank: The solubility of gases in water ________ with increasing temperature.

Answer 7

decreases

Question 8

What is the significance of the ion product (Q) in relation to the solubility product constant (Ksp)?

Answer 8

If Q < Ksp, the solution is unsaturated and no precipitation will occur. If Q > Ksp, precipitation will occur until Q = Ksp.

Question 9

What is the common unit for expressing solubility?

Answer 9

g/L or mol/L

Question 10

What is the difference between molar solubility and solubility?

Answer 10

Molar solubility is the number of moles of solute that can dissolve in a liter of solvent, while solubility is the maximum amount of solute that can dissolve in a given quantity of solvent.

Question 11

The common ion effect

Answer 11

The shift in the position of an equilibrium upon addition of a substance that
provides an ion in common with one of the ions already involved in the equilibrium