[Howard610]

I have a question on a problem, it starts out as "Can H(+)(aq) oxidize Sn(s)" I said yes and wrote the following equation

2H(+)(aq) + Sn(s) <---> Sn(2+) + H2

the next part says find the Ecell. Which i found to be .1364V because E(reduction H+) = 0v and E(oxidation Sn) = .1364V.

The next part asks to find the Ecell if the Ph is 5.39 and both the H2 and Sn(2+) concentrations are 1.5M. Would I use the Nernst equation to find this out?

Thanks

[Borek]

The next part asks to find the Ecell if the Ph is 5.39 and both the H2 and Sn(2+) concentrations are 1.5M. Would I use the Nernst equation to find this out?

Yes.

[Howard610]

where does pH fit into the nernst equation? If the nernst equation is

E=Ecell-(RT/nF)lnQ

i might have figured it out, since the pH is 5.39 meaning the H+ concentration is log(5.39)=.7315887M. then for lnQ=[Sn(2+)]/[H(+)]
substitute in the concentrations of Sn(2+) is 1.5M and H(+) is .7315887M. when putting it into the nernst equation, would i double the concentration of H(+) since there is 2moles of H(+) in the equation?

[Borek]

Q

[Howard610]

Borek i might have figured it out, since the pH is 5.39 meaning the H+ concentration is log(5.39)=.7315887M. then for lnQ=[Sn(2+)]/[H(+)]
substitute in the concentrations of Sn(2+) is 1.5M and H(+) is .7315887M. when putting it into the nernst equation, would i double the concentration of H(+) since there is 2moles of H(+) in the equation?

[Borek]

http://en.wikipedia.org/wiki/Reaction_quotient