Calculate pH of 0.10mol/L FeSO4(s) in Distilled Water

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The pH of a 0.10 mol/L solution of FeSO4 in distilled water is influenced primarily by the hydrolysis of Fe2+ ions. The sulfate ion (SO42-), being the conjugate base of the strong acid H2SO4, does not affect the pH. The hydrolysis of Fe2+ leads to a slight increase in acidity, with a dissociation constant (Ka) of 1.8 x 10-7. Additionally, the formation of Fe(OH)2, which is weakly soluble, may further lower the pH.

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How do i find the pH of FeSO4(s), knowing that its concentration is 0.10mol/L
it is a salt.. and it was placed in distilled water..FeSO4---->< Fe+2 + SO4-2

SO4-2 is the conjugate base of a strong acid H2SO4- therefore SO4-2 has no effect on the pH

in this case what is Fe+2,would be an acid and the Ka is equla to 1.8*10^-7
then i would combine Fe with h2o
and then what will the equation be?
 
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SO42- will hydrolize slightly - giving HSO4-, raising pH.

Fe(OH)2 is weekly soluble, so it may lower pH.

Finding exact answer may be a little bit tricky.
 
Last edited:

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