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Sagot :
Molar solubility of Fe(oh)3 in a solution that is buffered at pH 2.50 is 2.0×10−3M.
What is solubility product constant?
A salt compound will dissolve in the liquid water by forming an aqueous solution of its constituent ions. The saturated solution has compound dissociation reaction in a solubility equilibrium and we define this state using the compound's solubility product constant Ks p . This parameter will only change with solution temperature. In contrast, compound's molar solubility limit in the saturated solution can be manipulated in numerous other methods. One example involves trying to dissolve an acidic/basic salt compound in a solution that is buffered at certain pH . The pH will control compound's molar solubility because it affects the molarity of the acidic/basic constituent ion in the solution.
How can we solve it?
Iron (III) hydroxide has following solubility equilibrium for its saturated solution with the given constant value:
Fe(OH)3(s)⇋Fe3+(a q)+3OH−(a q)
Ks p=6.3×10−38=[Fe3+][OH−]3
From the given pH we find hydroxide ion molarity:
pH=2.50
pOH=14.00−2.50=11.50[OH−]=10−pOH=10−11.50=3.2×10−12 M
It is assumed that the iron (III) hydroxide makes a negligible contribution to hydroxide ion molarity. We solve the expression for molar solubility of this compound x:
Ks p=6.3×10−38=(x)(3.2×10−12 M)3
x=2.0×10−3M
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