Question

1)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

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

3) For any pair of solids. does the one with the largest Ksp always have the larger solubility? Why or why not?

*List cation (M), anion (M), molar solubility (M) and Ksp*

Design experiments in the virtual lab to answer the follow questions, 1). Use the virtual lab to determine the solubility product (Ksp) for the following solids: (a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2 2 1.5x100 S = 1.27x10-4 a) Kop c) Ksp = (29) ² x $=45° = 8-1x102 s=71.8x10o = 1.34*10-smolle (8.1x10-12 b) Ksp = 5x (25)² =493 = 1.14x10? v3.5*100 = 5.92x104 mol, =3.05*10-3 mol/L) samoly d) kse s? = 3.5810) S (1.1481o- 4 2). What is the solubility of the solids listed in problem 1, in grams liter" grams per liter)? 3). For any pair of solids, does the one with the largest Ksp always have the larger solubility? Why or why not?

Answer 1

As per HOMEWORKLIB RULES I have answered only question 1

Plzz upvote

Tq.....