The Ksp for Cu (OH) 2 is 4.8 * 10-20. Determine the molar solubility of Cu (OH) 2 in a buffer solution with a pH of 10.1.

A) 6.0 * 10-10

B) 7.6

C) 2.2 * 10-10

D) 3.8 * 10-16

E) 3.0 * 10-12

E) 3.0x10⁻¹²

Explanation:

Ksp of Cu (OH) ₂ is defined as:

Cu (OH) ₂ (s) ⇄ Cu²⁺ (aq) + 2 OH⁻ (aq)

Ksp = [Cu²⁺] [OH⁻]²

When pH is 10.1, [OH⁻] is:

pOH = 14 - pH

pOH = 3.9

pOH = - log [OH⁻]

[OH⁻] = 1.26x10⁻⁴M

Replacing in ksp formula:

4.8x10⁻²⁰ = [Cu²⁺] [1.26x10⁻⁴]²

3.0x10⁻¹² = [Cu²⁺]

That means the maximum amount of Cu²⁺ that can be in solution is 3.0x10⁻¹²M, thus, molar solubility of Cu (OH) ₂ is

E) 3.0x10⁻¹²