Suppose a solution contains 0.27 M Pb2 and 0.45 M Al3 . Calculate the pH range t

Question

Suppose a solution contains 0.27 M Pb2 and 0.45 M Al3 . Calculate the pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp values for Al(OH)3 is 4.6*10^-33 and Pb(OH)2 is 1.43*10^-20

Minimum ______ <pH< ________ Maximum

No clue how to do this.


Al(OH)3 (s) -> Al^3+(aq) + 3OH^-(aq)

Pb(OH)2 (s) -> Pb^2+(aq) + 2OH^- (aq) Suppose a solution contains 0.27 M Pb2 and 0.45 M Al3 . Calculate the pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp values for Al(OH)3 is 4.6*10^-33 and Pb(OH)2 is 1.43*10^-20

Minimum ______ <pH< ________ Maximum

No clue how to do this.


Al(OH)3 (s) -> Al^3+(aq) + 3OH^-(aq)

Pb(OH)2 (s) -> Pb^2+(aq) + 2OH^- (aq)

Explanation / Answer

Pb(OH)2 (s) -> Pb^2+(aq) + 2OH^- (aq)

k = [Pb2+]*[OH-]^2 / [Pb(Oh)^2]

k = (0.27) /(1.43*10^-20)

k = 1.88 * 10^19

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.