Question

2)Use the virtual lab to determine the solubility product (Ksp) for the following solids. Show all work for credit. *should be able to use the lab to determine the ion concentrations at equilibrium and use these for the formulas for KSP and then the KSP'S for solubility. The lab is just to help you get the ion concentration

(a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2

3) What is the solubility of the solids listed in question 2, in moles/liter? (1 mark each)

(i am so confused on what to do)

Answer 1

ANSWER:

Remember that solubility is an equilibrium phenomena that indicates the maximum amount of solute that you can dissolve in the solvent. Or, the amount of solute needed to prepare a saturated solvent.

If the system is at equilibrium the solution must be saturated. Then, the K_sp (equilibrium solubility product) could be used to find the solubility of any salt.

NOTE: The K_sp values change sligthly from one book to another. Please verify the K_sp values used for your virtual lab

1) AgCl

• The K_sp of AgCl is 1.8x10^-10
• The solubility reaction is

• And the K_sp expression is

• At the equilibrium

	AgCl	<---->	Ag+	+	Cl-
Equilibrium			s		s

• The solubility of AgCl will be equal to the concentration of Ag⁺

2) SrSO₄

• The K_sp of SrSO₄ is 3.5x10^-7
• The solubility reaction is

• And the K_sp expression is

• At the equilibrium

	SrSO4	<---->	Sr+2	+	SO4-2
Equilibrium			s		s

• The solubility of SrSO₄ will be equal to the concentration of Sr⁺²

3) Ag₂CO₃

• The K_sp of Ag₂CO₃ is 8.1x10^-12
• The solubility reaction is

• And the K_sp expression is

• At the equilibrium

	Ag2CO3	<---->	2 Ag+	+	CO3-2
Equilibrium			2s		s

• The solubility of Ag₂CO₃ will be equal to the concentration of CO₃^-2

4) Sr(IO₃)₂

• The K_sp of Sr(IO₃)₂ is 1.14x10^-7
• The solubility reaction is

• And the K_sp expression is

• At the equilibrium

	Sr(IO3)2	<---->	Sr+2	+	2 IO3-
Equilibrium			s		2s

• The solubility of Sr(IO₃)₂ will be equal to the concentration of Sr⁺²