kingkey24 Posted April 15, 2013 Posted April 15, 2013 (edited) Here is the problem: 50.00 mL of an aqueous solution which is 0.0525 M in sodium phosphate is titrated with an aqueoussolution which is 0.100 M in ferrous chloride. Calculate the solubility of ferrous phosphate whenenough 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 April 15, 2013 by kingkey24
John Cuthber Posted April 15, 2013 Posted April 15, 2013 There isn't enough information to answer that question. Was any other information given?
kingkey24 Posted April 15, 2013 Author Posted April 15, 2013 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
Recommended Posts
Create an account or sign in to comment
You need to be a member in order to leave a comment
Create an account
Sign up for a new account in our community. It's easy!
Register a new accountSign in
Already have an account? Sign in here.
Sign In Now