Electrolytic Solution Conductometry
CONDUCTOMETRY
1.0 Definition
Conductometry is basically a method which is used for the measurement of conductivity with respect to relative electrodes in ionic solutions that have an electric field.
OR
It can also be defined as the instrument through which we can find the electrical conductivity of an electrolytic solution.
2.0 Unit: It can be measured in mhos (Ωˉ1).
3.0 Electrical conductivity of an electrolytic solution based upon:
Ions numbers: Larger the conductivity of a solution, if it contains greater numbers of ions in it.
Temperature: As we increase the temperature the conductivity of a solution also goes on increasing, as it depend upon the ion temperature ranges from the 1 to 9% / Kelvin.
Viscosity: The viscosity decreased,
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Specific conductance (K):
The electrolytic solution conductivity is basically a measure to its capability to conduct the current. Its SI unit is S/m.
It is basically used in industries where it is use to measure the water purification through the water purification systems. Molar conductance: (ˆ)
The measurement of conductance of any solution that have one mole of the solute in Vcc of solution that are present between the two parallel electrodes that are present from 1 cm aside. It can be define like that as the electrolytic solution conductivity will be divided by molar concentration of an electrolyte, and the measurement of the productivity with which a bestowed electrolyte conducts electricity in a solution. Units are Siemens / meter per molarity, and the symbols used commonly are Λ or Λm Equivalent conductance: (^eq)
The strength of conducting all the ions formed by dissolving one gram equivalent in the solution of an electrolyte. The unit of equivalent conductance are the Resistance: (R)
The measurement of conductors opposition to the flow of electric
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