± Common-Ion Effect on Solubility for Lead Thiocyanate Lead thiocyanate, Pb(SCN ) 2 Common-Ion Effect Consider...

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± Common-Ion Effect on Solubility for Lead Thiocyanate Leadthiocyanate, Pb(SCN ) 2 Common-Ion Effect Consider the dissolutionof AB(s) : AB(s)⇌A+(aq)+ B − (aq) Le Châtelier's principle tells usthat an increase in either [ A + ] or [ B − ] will shift thisequilibrium to the left, reducing the solubility of AB . In otherwords, AB is more soluble in pure water than in a solution thatalready contains A + or B − ions. This is an example of thecommon-ion effect. Part B Calculate the molar solubility of leadthiocyanate in 1.00 M KSCN . Express your answer with theappropriate units. , has a K sp value of 2.00× 10 −5 .

Part A Calculate the molar solubility of lead thiocyanate inpure water. The molar solubility is the maximum amount of leadthiocyanate the solution can hold. Express your answer with theappropriate units.

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3.9 Ratings (660 Votes)

PbSCN (s) < ----------> Pb2+ (aq.) + 2 SCN- (aq.)

S                                S                2S    Mol/L of solubility

Ksp = [Pb2+][SCN-]2

In pure water,

2.00 * 10-5 = (S)(2S)2

2.00 * 10-5 = 4S3

S = (2.00 *10-5 / 4 ) 1/3

S = Solubility of lead thiocyanate in pure water = 2.236 * 10-3 M

In KSCN solution,

KSCN -------------> K+ (aq.) + SCN- (aq.)

1.00                    1.00         1.00M

[SCN-] = 1.00 M Since KSCN is completely soluble assume the [SCN-] is approximately equals to conc. of SCN- coming from KSCN.

therefore,

Ksp = [Pb2+]SCN-]2

2.00 * 10-5 = (S)(1.00)2

S = solubility of lead thiocyanate in 1.00 M KSCN solution = 2.00 * 10-5 M


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