Question

1) The hydroxide ion concentration of a saturated solution of Fe(OH)2 is 1.6X10^-5M. What is the...

1) The hydroxide ion concentration of a saturated solution of Fe(OH)2 is 1.6X10^-5M. What is the solubility product constant for Fe(OH)2?

2)What is the Kb for the following equilibrium? Ka for HNO2 is 5.0X10^-4.; No2- + H2O --> HNO2 + OH-

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Homework Answers

Answer #1

1)

[OH-] = 1.6 x 10^-5 M

Fe(OH)2 <-----------------------> Fe+2    +   2OH-

                                              0.8 x 10^-5      1.6 x 10^-5 M

Ksp = [Fe+2][OH-]^2

Ksp = (8 x 10^-6 ) (1.6 x 10^-5)^2

Ksp = 2.05 x 10^-15

solubility product constant = Ksp = 2.05 x 10^-15

2)

Ka = 5.0 x 10^-4

Kb = Kw / Ka

Kb = 1.0 x 10^-14 / 5.0 x 10^-4

Kb = 2.0 x 10^-11

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