Monday
November 24, 2014

Homework Help: chemistry

Posted by Tanner on Sunday, March 25, 2012 at 5:19pm.

Both Fe2+ and Cd2+ are precipitated by sulfide. However, they can be quantitatively separated through pH adjustment. You are given a solution containing 0.086 M Fe2+ and 0.062 M Cd2+. Calculate the [H+] range for a saturated H2S solution (ie, [H2S]=0.10 M) in which at least 99.99% of the least soluble ion can be precipitated while the other remains entirely in solution. The relevent equilibria are:
FeS(s) Fe2+ + S2‾ Ksp = 4.9 10-18
CdS(s) Cd2+ + S2‾ Ksp = 3.6 10-29
H2S(aq) 2 H+ + S2‾ Ka12 = 1.3 10-20

What is the lower limit [H+] of the separation range at which the most soluble ion will begin to precipitate?

What is the upper limit [H+] of the separation range at which 99.99% of the least soluble ion will remain precipitated?

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry. - a quantity of 25 ml of a solution containing both Fe2+ and Fe3+ ...
Chemistry - when 25.0 mL of a solution containing both Fe2+ and Fe3+ ions is ...
chemistry - A 49.45 mL sample of solution containing Fe2+ ions is titrated with ...
chemistry - Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to ...
Chemistry/Electrochem - Consider a cell at 299K: line notation Fe-Fe2+(1.39)--...
chem- IP and Ksp - A solution with a pH=6.00 is 4.0E-3M in each of the metal ...
chemistry - exam practice help!! - For the cell shown below, which will increase...
chemistry - balance the net ionic equation for the overall reaction. Pt | Fe2+(...
chemistry - 25.0 cm3 of an acidified solution containing Fe2+ ions was titrated ...
Chemistry - How many milliliters of a 3.85 M solution of Fe2+ are needed to ...

Search
Members