Finding out % of As2O3 in a sample

[ssb]

1. The problem statement, all variables and given/known data

A 3.67 gram sample of bug spray was decomposed in acid. Any As^5^+ was reduced to As^3^+ and diluted to 250.0 mL in a volumetric flask. A 5.00 mL sample of this was added to 125.0 mL of 0.0500 M KI buffered to pH 7. A coulmetric titration was carried out with electrically generated I_3^-, which oxidized As^3^+ to As^5^+ according to the reaction:

As^3^+ + I_3^- ----> 3I^- + As^5^+

The titration required 287 seconds at a constant current of 24.28 mA to reach the endpoint. Calculate the percentage of As_2O_3 (197.84 g/mol) in the bug spray.

2. Relevant equations

Moles Reacted = (I*t)/(nF)

3. The attempt at a solution

moles reacted = (.02425 amps * 287 seconds)/(2 (# electrons) * 9.6482x10^4 (Faraday constant)

moles reacted = 3.607x10^-^5

Question 1) Am I right to assume it is a one to one ratio of moles? or is it a one to 3 ratio? Assuming its one to one then (3.607x10^-^5) * (197.84 g/mol) = 7.136x10^-^3 grams of As_2O_3
If you divide this by the original mass (7.136x10^-^3)/(3.67g) oh and multiply by 100 to calculate percent, I come up with 0.1944%. NOW: I was able to do this with about half of the information given in the original equation. I looked at sample problems in my book and found similar calculations can be done if you are given standard potentials for half reactions. We were given none and I cannot find a standard potential for As^3^+ ----> As^5^+ + 2e^-

Question 2) where am I going wrong here? Thank you so much whoever is able to help me tackle this homework problem

[Borek]

Iodine works only as an intermediate in transfering charge, so you may simply assume reaction going is As3+ -> As5+ + 2e- - you know how to calculate the charge, you should be eable to calculate amount of As.

As moles number seems correct, but it is not identical to the number of moles of As2O3.

You forgot that sample was diluted and only part was titrated.

[ssb]

Iodine works only as an intermediate in transfering charge, so you may simply assume reaction going is As3+ -> As5+ + 2e- - you know how to calculate the charge, you should be eable to calculate amount of As.

As moles number seems correct, but it is not identical to the number of moles of As2O3.

You forgot that sample was diluted and only part was titrated.

moles reacted = (.02425 amps * 287 seconds)/(2 (# electrons) * 9.6482x10^4 (Faraday constant)

Moles reacted = 3.607 x 10^{-22}

Since its a 1 to 1 ratio of mol As^{3+} to mol I_3 then there are also 3.607 x 10^{-22} mol of I_3

So I will now solve for grams of As_2O_3

Grams As_2O_3 = (3.607 x 10^{-22}/5.00 mL) * (250 mL) * (1 mol As_2O_3/2 mol As^{3+}) (197.84 grams / mol As_2O_3) = 0.178 grams

0.178 grams / 3.67 grams (original sample size) = .0485

.0485 (100) **percentage calculation** = 4.85%

Does this look good?

[Borek]

Much better now.