a. The cations Ba^2+ and Sr^2+ can be precipitated as very insoluble sulfates. I

Question

a. The cations Ba^2+ and Sr^2+ can be precipitated as very insoluble sulfates. If you add sodium sulfate to a solution containing these metal cations, each with a concentration of 0.17 M, which is precipitated first: BaSO_4 or SrSO_4 (K_sp for BaSO_4 is 1.1 times 10^-10, K_sp for SrSO_4 is 3.4 times 10^-7)? BaSO_4 SrSO_4 b. The cations Ba^2+ and Sr^2+ can be precipitated as very insoluble sulfates If you add sodium sulfate to a solution containing these metal cations, each with a concentration of 0.17 M, what will be the concentration of the a first ion that precipitates (Ba^2+ or Sr^2+) when the second, more soluble salt begins to precipitate? (K_sp for BaSO_4 is 1.1 times 10^-10, K_sp for SrSO_4 is 3.4 times 10^-7)?

Explanation / Answer

[Sr+2] = 0.17 M

Ksp of BaSO4 is less than Ksp of SrSO4. so BaSO4 is ready to precipitate and SrSO4 is ready to soluble .

SrSO4 -----------------------> Sr+2 + SO4-2

Ksp = [Sr+2][SO4-2]

3.4 x 10^-7 = 0.17 [SO4-2]

[SO4-2] = 2.0 x 10^-6 M

now BaSO4

BaSO4 ----------------------> Ba+2 + SO4-2

Ksp = [Ba+2] [SO4-2]

1.1 x 10^-10 = [Ba+2] x 2 x 10^-6

[Ba+2] = 5.5 x 10^-5 M

3.4 x 10^-7 =

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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