Determine the molar solubility of Al(OH) 3 in a solution containing 0.0500 M AlC

Question

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3.

Ksp (Al(OH)3) = 1.3 × 10-33.

6.5 x 10-35 M

1.04 x 10-29 M

2.6 x 10-9M

5.2 x 10-31 M

2.6 x 10-32 M

Please help with this problem, I have even gotten 9.87 x 10-12 from:

Ksp = s(3s)3

= 1.3 x 10-33 = 0.05(3s)3

= 2.6 x 10-32 = (3s)3

= 2.0 x 10-11 = 3s

= 9.87 x 10-12 M = s

(and also the answer is NOT s= 2.6 x 10-9 M)

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3.

Ksp (Al(OH)3) = 1.3 × 10-33.

6.5 x 10-35 M

1.04 x 10-29 M

2.6 x 10-9M

5.2 x 10-31 M

2.6 x 10-32 M

Explanation / Answer

Al(OH)3 <-> Al+3 + 3OH-

Ksp = [Al+3][OH-]^3

[Al+3] already in solution = 0.0500

then

Ksp = (0.0500 )(3S)^3

1.3*10^-33= (0.0500 )(3S)^3

S = ((1.3*10^-33)/(0.05)/27)^(1/3) = 9.8749*10^-12 M

Related Questions

Navigate

• Browse (All)
• Browse D
• Subjects

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