Did you square the 0.019*2 for B^-?
........AB2 ==> A^2+ + 2B^-
I......solid....0.......0
C.....-0.0190..0.019..0.019*2
E......solid...0.019..0.038
Ksp = (A^2+)(B^-)^2
Ksp = (0.019)(0.038)^2
Ksp = 2.74E-5 for the answer. I do it slightly different because it's faster on the calculator.
Ksp = (A^2+)(B^-)^2
Kso = (x)(2x)^2 = 4x^3
Ksp = 4*(0.019)^3 = 2.74E-5.
The usual student mistake is to double the 0.019 to find B^- but forget it is squared.
At 25C only .0190 mol of the generic salt AB2 is soluble in 1.00L of water. What is the Ksp of the salt at 25C?
AB2<->A^2+ + 2B^-
I took the .0190 mol and doubled it and multiplied by .019 again and got 6.859x10^-6 and got it wrong what should I do?
Please help Dr. Bob
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