Solubility of Cr hydroxide in buffered solution

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SUMMARY

The solubility of chromium hydroxide (Cr(OH)3) in a buffered solution at pH 8.673 is determined using its solubility product constant (Ksp) of 30.220, which corresponds to a Ksp value of 6.0256 E -31. To find the solubility in grams per liter, one must first calculate the hydroxide ion concentration ([OH-]) from the pOH derived from the given pH. Subsequently, this [OH-] value is used in the Ksp equation to find the concentration of chromium ions ([Cr+3],) which can then be converted to grams of Cr(OH)3.

PREREQUISITES
  • Understanding of solubility product constant (Ksp) calculations
  • Knowledge of pH and pOH relationships
  • Familiarity with stoichiometry in chemical equations
  • Basic concepts of buffered solutions
NEXT STEPS
  • Calculate the pOH from the given pH of 8.673
  • Determine the concentration of hydroxide ions ([OH-]) using the pOH
  • Apply the Ksp expression to find the concentration of chromium ions ([Cr+3])
  • Convert the concentration of [Cr+3] to grams of Cr(OH)3 using its molar mass (103.02 g/mol)
USEFUL FOR

Chemistry students, particularly those studying solubility equilibria, environmental scientists analyzing chromium compounds, and educators preparing materials on chemical equilibria.

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Homework Statement


What is the solubility (gram/liter) of Cr(OH)3 (103.02 g/mol) in a solution buffered at pH = 8.673? The pKsp of Cr(OH)3 is 30.220.


Homework Equations


Ksp = [Cr][OH]^3
Cr(OH)3 -> Cr + 3OH


The Attempt at a Solution


I have already solved that Ksp = 6.0256 E -31, but I'm not entirely sure what to do with the buffer pH. I tried using it to find the pOH and subsequently [OH], but for some reason I'm not getting the right answer. Do I plug [OH] into the Ksp equation after finding out the concentration using the pH or is there a step I'm missing?
 
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Sounds like you are approaching it correctly. Use the concentration of [OH-] you obtain from the pOH in the Ksp expression and determine [Cr+3]. From that revelation back out how many grams of Cr(OH)3 will produce that concentration of [Cr+3].
 

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