Electrochemistry and liquid junctions

AI Thread Summary
The discussion centers on the electrochemical system involving Pt(s)/H2(g)/HBr(aq)/AgBr(s)/Ag(s) and the necessity of a liquid junction. It is clarified that AgBr is insoluble in water, leading to a saturated solution containing minimal Ag+ ions, which are reduced on the electrode. The slow reaction between H2 and Ag+ is deemed negligible, not affecting the cell potential. The lack of mixing between H2 and the Ag+ and Br- ions further supports the conclusion that a liquid junction is unnecessary. Overall, the system's dynamics allow for effective electrochemical reactions without the need for a liquid junction.
badbrain103
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I have Pt(s)/H2(g)/HBr(aq)/AgBr(s)/Ag(s)

The question asks why a liquid junction is not necessary. So I know AgBr is insoluble in water, and AgBr coats the silver metal. I just don't understand why it does not matter that the Br- anions from AgBr mixing with the H+ cations doesn't necessitate a liquid junction. Any help?
 
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Write net ionic reaction equation.
 
well the two half reactions are:
H2 --> 2H+ + 2e-
2AgBr(s) + 2e- --> Ag(s) + Br-

giving the net ionic equation:

H2 + 2AgBr --> 2H+ + 2Ag(s) + 2Br-

there are no spectator ions...
so...?
 
badbrain103 said:
H2 + 2AgBr --> 2H+ + 2Ag(s) + 2Br-

This is not exactly true. That is - what is really happening is that the solution is saturated with AgBr - so it contains some minute amounts of Ag+. This Ag+ gets reduced directly on the electrode. In theory it can also get reduced by hydrogen in the bulk of the solution, but as concentration of Ag+ is very small, this reaction would be pretty slow. Besides, once the Ag+ is removed from the solution, it has to saturate it again - this dissolution is another pretty slow process. Then, electrode is covered with wet AgBr in which transport of H2 is very slow (no mixing). Thus we can safely assume there is no hydrogen "below" AgBr, just solution containing Ag+ and Br-.
 
Ok sorry I haven't done electrochemistry in a long time and am a bit confused. So the solution is of AgBr mostly though it contains some small amount of H2 and Ag+ - this is because most of the Ag+ is reduced quickly, right?

Because the reaction between H2 and Ag+ is so slow, it is basically negligible and does not affect the cell potential at all, is this right?

What do you mean when you said the Ag+ is removed from the solution - that the majority of it is reduced to become Ag(s)?

But finally, because there is no mixing between H2 and the Ag+ and Br-, it is safe to assume that this does not affect the cell potential, thus why there is no need for a liquid junction?
 
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