Recent content by OmniReader

Currents very tiny, so would take long for equilibrium to be reached. but still why fast electrode kinetics are desirable then?

so statement "Fast electrode kinetics is desirable" is incorrect, we desire to see the initial emf. also isn't this destructive, we our method for reading concentrations is changing them... I think I have grasped voltmeter concept from my book.

ok, closed circuit allows transfer of electrons between the solutions so redox reaction occurs. this changes conc of species, so how does emf not change down to 0. as, won't it disturb emf reading, if you control or interfere the natural redox flow of electrons? but if you don't redox...

Proton concentration cell is made by connecting with Pt wire two acid-base solutions and measuring emf. but wire allows redox reaction, changing conc of H+ in each solution. how is original pH found- with initial emf reading?

have read books, none cover the issue. please sugest good title or provide link. I maybe know why. emf reading is taken for K or conc measurement, not needed to do so in cases when different redox are possible. instead conc is made small for non-main redox and then discarded so "only main"...

constant=F. I googled Faraday's laws.question is: what about situation in which are few possible redox reactions, e.g. aqueous solution. Which is chosen at cathode and anode respectively? same question for EMF in fact ...

please specify calculations: what quantity current will be drawn by cell . Or constant-current transfers what quantity of mass. is irreversibility approximation made? for approximation "only 1reduction and 1 oxidation reaction", how is it chosen when solution has many redox reactions?

I didnot know. this Please provide links w/detailed info& calculations.

now I understand. redox reaction occurs without electrode too, only purpose of electrode is to measure K/conc. can we apply quantitative equilibrium method to solutions w/redoxreactions?

ok so for my last example is Pb(s) | PbSO4(s) | K2SO4(aq) || KNO3(aq) || KCl(aq) | PbCl2(s) | Pb(s) the reactions will be PbSO4 (s) + 2e- = Pb(s) + SO4^2-(aq), PbCl2(s) + 2e- = Pb(s) + 2Cl-(aq), overall. for example Fe (s) | Fe(OH)3(s) | NaOH (aq) reaction will be Fe(OH)3(s) + 3e- = Fe(s) +...

I thought reaction would be AgCl(s) + e- = Cl-(aq) + Ag(s). So if "solid"(s) salt (or known for low solubility) is there we must use Ksp equation?

and for salts who don't dissociate/dissolve, AKA with solid state symbol (solubility rules tells us), e.g. Hg2Cl2, PbSO4, PbCl2, list goes on including from examples used. what reactions for the solid salts, or those like Hg2Cl2 that dissolve but not dissociate?

Please tell me how to deduce reliably from galvanic cell representation, the half-cell reactions, for any cell, or vice versa. Pt(s) | H2(g) | HCl(aq) | Cl2(g) | Pt(s) Pb(s) | PbCl2(s) | HCl(aq) | H2(g) | Pt(s) Pb(s) | PbSO4(s) | K2SO4(aq) || KNO3(aq) || KCl(aq) | PbCl2(s) | Pb(s)...

Thanks, I have another problem. I want to know how to deduce reliably from galvanic cell representation, the half-cell reactions, for any cell, or vice versa. Pt(s) | H2(g) | HCl(aq) | Cl2(g) | Pt(s) Pb(s) | PbCl2(s) | HCl(aq) | H2(g) | Pt(s) Pb(s) | PbSO4(s) | K2SO4(aq) || KNO3(aq) || KCl(aq)...

is the complete robust method to not use standard potentials but rather convert all potentials and equilibrium constants into standard Gibbs' free energy using the Delta Gº = -n * F * Eº and Delta Gº = -R * T * ln(K) relations after which the Delta Gº values are completely additive, and then...