Question
In: Chemistry
Consider the following equilibrium: Fe(OH)3(s) D Fe3+(aq) + 3OH–(aq) with Ksp = 1.6 x 10-39. The...
Consider the following equilibrium: Fe(OH)3(s) D Fe3+(aq) + 3OH–(aq) with Ksp = 1.6 x 10-39. The activity coefficients for Fe3+(aq) and 3OH–(aq) are 0.445 and 0.900 in a solution with an ionic strength of 0.01M. The pH of the solution was 11.
a. Calculate [OH–] in the solution.
b. Use the activity coefficients in order to calculate [Fe3+] in the solution.
Solutions
Expert Solution
Ionic strength:
Ionic strength is described as the estimation of solution’s entire ionic concentration. Ionic strength was introduced for the first time when ionic compound’s activity coefficients were being studied.
__Given Data:__
*The 
of 
is 
*The activity coefficient of
is 0.445
*The activity coefficient of
is 0.900
*The ionic strength is 0.01 M
*The pH of the solution is 11
__Explanation to part a:__
The formula written below is used
for calculating 
Substitute the given values in the
equation above in order to evaluate the 
The calculation for
is shown below
Therefore, the concentration of
in the solution is 
__Explanation to part b:__
The dissolution
of
is shown below.
The solubility product expression
for
is written in the following manner.
In the above equation (I) 
and 
are the activity coefficients.
The known values are substituted in
the equation (I) above in order to evaluate 
ion concentration
Therefore, the concentration of
in the solution is 
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