Assignment 4 - K a1 =5.8x10-3 , K a2 =1.10x10-7 , K a3...

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Quantitative Analysis Assignment #4 Due 10/25/04 Systematic Treatment of Equilibria 1) During the late 1800s and through the mid 1900s, arsenates were frequently used as insecticides. They were sparingly soluble in water with pH near neutral. However, with either low or high pH, they were much more soluble and could get into the water through interaction with other equilibria, resulting in arsenic in the drinking water. Lead arsenate (Pb 3 (AsO 4 ) 2 ) has a solubility product of 4.29x10 -13 . Arsenic acid (H 3 AsO 4 ) is a triprotic acid with
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Unformatted text preview: K a1 =5.8x10-3 , K a2 =1.10x10-7 , K a3 =3.2x10-12 . In solution, lead can precipitate out with a high enough hydroxide concentration. ( K sp =4.2x10-15 ) However, lead can also form up to four complexes (3 charged, 1 neutral) with hydroxide ion. The formation constants are: K f1 =2.45x10-3 , K f2 =1.36x10-4 , K f3 =3.31x10-7 , K f4 =3.22x10-2 . Use the systematic treatment through step 5 to setup how you would solve this equilibrium problem. (Note: you do not need to solve or attempt to solve this problem!)...
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This note was uploaded on 12/10/2008 for the course CHEMISTRY CHEM 3600 taught by Professor Philipj.silva during the Fall '07 term at Uni. Tartu.

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