The molar solubility of BaF2 is 6.29x10^-3 M. A. Write the solubility product co

Question

The molar solubility of BaF2 is 6.29x10^-3 M. A. Write the solubility product constant expression B. What is the Ksp value for BaF2 C. A decrease in pH will increase the solubility while an increase in pH has no effect. Explain. D. What could you add to the solution to form more precipitate? The molar solubility of BaF2 is 6.29x10^-3 M. A. Write the solubility product constant expression B. What is the Ksp value for BaF2 C. A decrease in pH will increase the solubility while an increase in pH has no effect. Explain. D. What could you add to the solution to form more precipitate? A. Write the solubility product constant expression B. What is the Ksp value for BaF2 C. A decrease in pH will increase the solubility while an increase in pH has no effect. Explain. D. What could you add to the solution to form more precipitate?

Explanation / Answer

BaF2(s) <-> Ba+2(aq) + 2F-(aq)

a.

Ksp = [Ba+2][F-]^2

b.

[Ba+2]= 6.29*10^-3 = 0.00629

[F-] = 2*6.29*10^-3 = 0.01258

Ksp = (0.00629)(0.01258^2) = 9.9543*10^-7

c.

F- + H+ <-> HF

therefore, adding H+ increases HF , decreases F-, makes the shift of BaF2 <-> toward products, that is, to solubilty

the reverse is true as well

d-

add SO4-2 contaning sallts such as Na2SO4

to precipitate BaSO4(s) , decrteasing Ba+2 ions, therefore, shift goes to more solid BaF2 toward Ba+2 and F-

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