Question

The molar solubility of Iron(III) hydroxide, Fe(OH)3 is 1.01 x 10-10 M. What is the solubility...

The molar solubility of Iron(III) hydroxide, Fe(OH)3 is 1.01 x 10-10 M. What is the solubility product constant, Ksp for this ionic compound in water?

My teacher got 2.81*10^-39. How is that correct?

Homework Answers

Answer #1

Solution :-

Given data

Solubiliy of the Fe(OH)3 = 1.01*10-10 M

Dissociation equation of the Fe(OH)3 is as follows

Fe(OH)3 -----> Fe3+ + 3OH-

Since mole ratio of the Fe(OH)3 to Fe3+ is 1 :1 therefore concentration of the Fe3+ =1.01*10-10 M

And mole ratio of the Fe(OH)3 to OH- is 1 :3 therefore concentration of the OH- = 3* [Fe(OH)3]

[OH-] = 3*1.01*10-10 M

           = 3.03*10-10 M

Lets write the ksp equation for this equation

ksp = [Fe3+][ OH-]3

now put the concentration values in the ksp formula

ksp = [Fe3+][ OH-]3

ksp = [1.01*10-10][ 3.03*10-10]3

ksp = 2.81*10-39

Therefore the answer given by the teacher is correct

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