Question

When you add 0.05 ml of 0.50M sodium thiosulfateNa2SO2O3 to 2.0 ml if 0.10M silvernitrate, a precipitate of Ag2S2O3 formed byequation 2Ag+ +S2O3-2 <------->Ag2(S2O3) (s) Assume that this reaction goes 100% to completion. a) Set up a reaction table and calculate the [Ag+] afterreaction b) Calculate the value of Ecell expected using Ag|([Ag+] from a) asthe test half-cell, and Ag+(1.0M)|Ag as the referencehalf-cell.

I don't have money to see answer, just a young man trying to succeed and save lives.

Answer 1

The final concentration for each ion is:

From the reaction:

	2Ag+	S2O32-	---->	Ag2(S2O3)
initial	0.098	0.012		0
after reaction	0.098-2*(0.012)	0.012-0.012		0.012

From the table you can see all S2O3 is going to be consumed

So the final concentration is 0.098-2*(0.012)=0.074M

b)

For the second, I do not understand what cell is it talking about, but you can calculate the potential of the half cell asuming Ag+ reduces to Ag

, since the standard potentials are calculated at 1M concentrations, Eo is the reference potential.