Solubility Equilibrium

Question 1

Solubility

Answer 1

Quantity of solute that dissolves in a given quantity of solvent at a particular temp

Question 2

Molar Solubility

Answer 2

The moles of solute that dissolve to make 1 L of a saturated solution

Question 3

Solubility Equilibrium

Answer 3

A Dynamic equilibrium between a solute and a solvent in a saturated in solution in a closed system. (both forward and backward reactions happening at the same rate.)

Question 4

Solubility Product Constant (Ksp)

Answer 4

The value obtained from the equilibrium law applied to a saturated solution. K=[product]

Question 5

What does Ksp tell you in terms of equilibrium?

Answer 5

The higher the Ksp value, the more soluble the compound is

Question 6

How is the formation of stalactites and stalagmites an example of solubility equilibrium?

Answer 6

A cave forms when groundwater containing atmospheric CO2, forming an acidic solution, dissolves limestone (CaCO3) in a process that may take tens of thousands of years. As groundwater seeps into a cave, water evaporates from the solution of CaCO3 in CO2-rich water, producing a supersaturated solution and a shift in equilibrium that causes precipitation of the CaCO3. The deposited limestone eventually forms stalactites and stalagmites.

Question 7

What does it mean when a compound that is insoluble on the solubility table?

Answer 7

A tiny amount of the compound will dissolve in water

Question 8

Trial Ion Product (Q) in relation to (K)

Answer 8

Q=K in equilibrium
Q>K dissolution equilibrium system sifts to the left/reactants (ppt forms)
Q

Question 9

Common Ion Effect

Answer 9

Reduction in the solubility of an ionic compound due to the solubility of an ionic compound ion solution

Question 10

What is the dissolving equation for Na2S (s)?

Answer 10

Na2S (s) -> 2 Na (aq) + S (aq)

Question 11

What is the dissolving equation for AgCl (s)?

Answer 11

AgCl (s) Ag (aq) + Cl (aq)