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Analytical Chemistry-Calculating Solubility Question

kingkey24
in Homework Help

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Here is the problem: 50.00 mL of an aqueous solution which is 0.0525 M in sodium phosphate is titrated with an aqueous
solution which is 0.100 M in ferrous chloride. Calculate the solubility of ferrous phosphate when
enough titrant has been added to be one milliliter past the equivalence point of the titration.

 

info: Iron(II) phosphate Ksp=1.0 x 10^-36

Iron(III) phosphate Ksp=4.0 x 10^-27

 

can someone help me get started with this? i am completely lost

Edited by kingkey24

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There isn't enough information to answer that question.

Was any other information given?

 

post edited with all relevant that was provided to me, there is no Ksp for Na3PO4 as it is very soluble

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