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Hatshy [7]
3 years ago
8

Lead thiocyanate, Pb(SCN)2, has a Ksp value of 2.00×10−5.a) Calculate the molar solubility of lead thiocyanate in pure water. Th

e molar solubility is the maximum amount of lead thiocyanate the solution can hold.b) Calculate the molar solubility of lead thiocyanate in 0.500 M KSCN.
Chemistry
1 answer:
kkurt [141]3 years ago
4 0

Answer:

a) 1.71 × 10⁻³ M

b) 8.00 × 10⁻⁵ M

Explanation:

In order to calculate the solubility (S) of Pb(SCN)₂ we will use an ICE chart. We identify 3 stages (Initial, Change, Equilibrium) and complete each row with the concentration or change in the concentration.

       Pb(SCN)₂(s) ⇄ Pb²⁺(aq) + 2 SCN⁻(aq)

I                                 0                   0

C                               +S               +2S

E                                 S                  2S

The solubility product (Ksp) is:

Ksp = 2.00 × 10⁻⁵ = [Pb²⁺].[SCN⁻]² = S . (2S)² = 4S³

S = 1.71 × 10⁻³ M

<em>b) Calculate the molar solubility of lead thiocyanate in 0.500 M KSCN.</em>

KSCN is a strong electrolyte that dissociates to give 0.500 M K⁺ and 0.500M SCN⁻.

       Pb(SCN)₂(s) ⇄ Pb²⁺(aq) + 2 SCN⁻(aq)

I                                 0                 0.500

C                               +S                +2S

E                                 S                0.500 + 2S

Ksp = 2.00 × 10⁻⁵ = [Pb²⁺].[SCN⁻]² = S . (0.500 + 2S)²

In the term (0.500 + 2S)², 2S is negligible.

Ksp = 2.00 × 10⁻⁵ = S . (0.500)²

S = 8.00 × 10⁻⁵ M

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