A solution is 0.10 M AgNO3 and 0.10 M Ba(NO3)2. If solid Na2SO4 is added to the

Question

A solution is 0.10 M AgNO3 and 0.10 M Ba(NO3)2. If solid Na2SO4 is added to the solution, what is [Ba2+] when Ag2SO4 begins to precipitate? (Ksp BaSO4 = 1.1 x 10-10; Ag2SO4 = 1.1 x 10-5)



1. 2.4 x 10-6 M

2. 1.0 x 10-7 M

3. 2.4 x 10-7 M

4. 3.2 x 10-6 M

5. 5.1 x 10-6 M

Explanation / Answer

When Na2SO4 is added to a solution of 0.10 M AgNO3 and 0.10 M Ba(NO3)2 Solid BaSO4 will precipitate first , Then , Solid Ag2SO4 will precipitate . You should know what is Ksp __ Solubility Product Constant For Solid BaSO4 BaSO4 Ba^2+ + SO4^2- Ksp = [ Ba^2+ ] x [ SO4^2- ] = 1.1 x 10^-10 For Solid Ag2SO4 - - - > Ag2SO4 2 Ag^+ + SO4^2- Ksp = [ Ag^+ ] x [ Ag^+ ] x [ SO4^2- ] = 1.1 x 10^-5 For Solid Ag2SO4 [ Ag^+ ] x [ Ag^+ ] x [ SO4^2- ] = 1.1 x 10^-5 [ 0.1 ] x [ 0.1 ] x [ SO4^2- ] = 1.1 x 10^-5 [ SO4^2- ] = 1.1 x 10^-3 For Solid BaSO4 [ Ba^2+ ] x [ SO4^2- ] = 1.1 x 10^-10 [ Ba^2+ ] x [ 1.1 x 10^-3 ] = 1.1 x 10^-10 [ Ba^2+ ] = 1.0 x 10^-7 So , ( B ) is the correct answer

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