Electrochemistry and liquid junctions

In summary, the liquid junction is not necessary because the Ag+ and Br- ions are not interacting with each other.
  • #1
badbrain103
4
0
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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  • #2
Write net ionic reaction equation.
 
  • #3
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...?
 
  • #4
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-.
 
  • #5
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?
 

FAQ: Electrochemistry and liquid junctions

What is electrochemistry?

Electrochemistry is a branch of chemistry that deals with the study of chemical reactions that involve the transfer of electrons and the production of electricity.

How do liquid junctions play a role in electrochemistry?

Liquid junctions are used in electrochemical cells to separate two different electrolyte solutions, allowing for the flow of ions between them and the production of an electric current.

What is the Nernst equation?

The Nernst equation relates the equilibrium potential of an electrochemical cell to the concentration of the reactants and products involved in the reaction. It is used to calculate the cell potential under non-standard conditions.

How do I determine the direction of electron flow in an electrochemical cell?

The direction of electron flow in an electrochemical cell can be determined by the relative potentials of the two electrodes. Electrons will flow from the electrode with a higher potential to the one with a lower potential.

What are some practical applications of electrochemistry?

Electrochemistry has many practical applications, such as in batteries, electrolysis processes, corrosion prevention, and sensors. It is also used in various industries, including metallurgy, pharmaceuticals, and environmental monitoring.

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