🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.
CH3NH2 → weak base
Step 1: Calculate OH‒ in the solution
Kb of CH3NH2 = 4.4×10‒4
x = 7.5754 × 10–3
x = –8.0154 × 10–3
x = [OH-]
[OH-] = 7.5754 × 10–3 M
Pb(OH)2(s) ⇌ Pb2+(aq) + 2 OH–(aq)
Ksp = 1.43×10‒20
What is the molar solubility of Pb(OH)2 in a 0.138-M solution of CH3NH2?
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