e) The molar solubility for compound MX2 equals 3.8 x 1012 M. What are the value

Question

e) The molar solubility for compound MX2 equals 3.8 x 1012 M. What are the values for [M] and [X]. What is Ksp? f) Calculate [Ag ] in a saturated aqueous solution of AgBr. [Ag+] Problem 4 (6 pts): Solubility and Precipitation When 10.00 mL of 1.00 M NaOH are added to 1.00 L of 0.100 M CaCl2 will a precipitate occur? Show you calculations. This is not a True/False question: Just answering "yes" or "no" is not a correct or acceptable answer Problem 5 (6 pts) Solubility and Le Chatelier's Principle What is the molar solubility of AgCl in 0.1 M HCI? How many grams of silver chloride will dissolve in 500 mL of 0.1 M HCI? Show all calculations.

Explanation / Answer

e) molar solubility of MX2 = 3.8x10-12 M

MX2 <------------> M+ + 2X-

s s 2s

Thus [M+2] = 3.8x10-12 M

and [X-] = 2x3.8x10-12 M

= 7.6 x10-12 M

Ksp = [M+2] {x-]2

= 3.8x10-12 M [7.6x10-12 M ]2

= 2.19 x10-22

f) ksp of AgBr = 5.0x10-13

AgBr <-------> Ag+ + Br-

s s s

Ksp = [Ag+][Br-]

= s2

Thus [Ag+] = [5.0x10-13]1/2

=7.07x10-7M

Problem 4

[OH-] in solution = 10mL x 1.0 /1010 mL

=0.0099

[Ca+2] in solution = 1000mL x 0.1/1010

=0.99 M

Ca(OH)2 <-----------> Ca+2 + 2OH-

Ksp = [Ca+2][OH-]2

Thus ionic product = [0.99](0.0099)2

= 9.7x10-5

Ksp of Ca(OH)2 = 2.5x10-14

As Ionic product > soluility product precipitation occurs.

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