Everything about Salt Bridge totally explained
» For the term used in protein chemistry, see Salt bridge (protein)
A
salt bridge, in
chemistry, is a laboratory device used to connect the
oxidation and
reduction half-cells of a
galvanic cell (voltaic cell), a type of
electrochemical cell. Salt bridge usually comes in two types: glass tube and
filter paper.
Glass tube bridges
One type of salt bridges consists of U-shaped glass tubes filled with a relatively inert
electrolyte, usually
potassium chloride or
sodium chloride.
Agar is often used for gelification.
The conductivity of the glass tube bridges depends mostly on the concentration of the electrolyte solution. An increase in concentration below
saturation increases conductivity. Beyond-saturation electrolyte content and narrow tube diameter may both lower conductivity.
Filter paper bridges
The other type of salt bridges consists of a filter paper, also soaked with a relatively inert
electrolyte, usually
potassium chloride or
sodium chloride because they're chemically
inert. No gelification agent is required as the filter paper provides a solid medium for conduction.
Conductivity of this kind of salt bridges depends on a number of factors: the
concentration of the electrolyte solution, the texture of the filter paper and the absorbing ability of the filter paper. Generally smoother texture and higher
absorbancy equates to higher conductivity.
A porous disk or other porous barrier between the two half-cells may be used instead of a salt bridge; however, they basically serve the same purpose.
Uses
As electrons leave one half of a galvanic cell and flow to the other, a difference in charge is established. If no salt bridge was used, this charge difference would prevent further flow of electrons. A salt bridge allows the flow of
ions to maintain a balance in
charge between the
oxidation and reduction vessels while keeping the contents of each separate. With the charge difference balanced, electrons can flow once again, and the reduction and oxidation reactions can proceed. In general, keeping the two cells separate is preferable from the point of view of eliminating
variables from an
experiment. When no direct contact between
electrolytes is allowed, there's no need to make allowance for possible interactions between ionic species.
The technique more specifically allows freedom in the choice of ions in
solution. For instance, a
mixture of two different cations in solution might result in the preferential reduction of the wrong one, for the purposes of the experiment. With a salt bridge, the desired cation is isolated in one vessel while the cation in the other vessel may be chosen to make the experiment easier, for example using a more soluble, or more stable salt of the anionic species.
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