Electrolytic Conduction
Electrolytic Conduction
Introduction
Electrical conductors can be classified into two types: (1) electronic conductors and (2) electrolytic conductors. Solid and molten metals, semiconductors, and some salts are examples of electronic conductors. Conduction takes place in electronic conductors by direct migration of electrons through the conductor under the influence of an applied potential. Here the atoms or ions that compose the conductor remain stationary (except for vibrations about their equilibirum positions) and these conductors carry a current as electrons pass through the orbitals of the atoms or ions. (See pages 449-501 in your text.)
Electrolytic conduction is observed in solutions of strong and weak electrolytes, in molten salts, and in some ionic solids. Conduction occurs in electrolytic conductors as both positive ions and negative ions migrate toward electrodes. In contrast to electronic conduction, electrolytic conduction involves a transport of ions from one part of the conductor to another. Further, the flow of current in an electrolytic conductor is accompanied by chemical changes at the electrodes. (Examples of such reactions can be found on pages 743 -747 of your text.) Electrolytic conduction plays an important role in the function of electrochemical cells, batteries, electrolysis, and electroplating.
We know that solutions can be nonelectrolytes (nonconductors), weak electrolytes (poor conductors), or strong electrolytes (good conductors). In this experiment we will determine the conductivity of such solutions in a more quantitative manner by measuring their conductance. We will examine how the conductivity of various solutions changes as the concentration and the identity of ions change. We will also see how conductivity can be used to follow chemical reactions.
Measuring Conductance The conductance of an electrolytic or electronic conductor is the reciprocal of its resistance in ohms. At one
Introduction
Electrical conductors can be classified into two types: (1) electronic conductors and (2) electrolytic conductors. Solid and molten metals, semiconductors, and some salts are examples of electronic conductors. Conduction takes place in electronic conductors by direct migration of electrons through the conductor under the influence of an applied potential. Here the atoms or ions that compose the conductor remain stationary (except for vibrations about their equilibirum positions) and these conductors carry a current as electrons pass through the orbitals of the atoms or ions. (See pages 449-501 in your text.)
Electrolytic conduction is observed in solutions of strong and weak electrolytes, in molten salts, and in some ionic solids. Conduction occurs in electrolytic conductors as both positive ions and negative ions migrate toward electrodes. In contrast to electronic conduction, electrolytic conduction involves a transport of ions from one part of the conductor to another. Further, the flow of current in an electrolytic conductor is accompanied by chemical changes at the electrodes. (Examples of such reactions can be found on pages 743 -747 of your text.) Electrolytic conduction plays an important role in the function of electrochemical cells, batteries, electrolysis, and electroplating.
We know that solutions can be nonelectrolytes (nonconductors), weak electrolytes (poor conductors), or strong electrolytes (good conductors). In this experiment we will determine the conductivity of such solutions in a more quantitative manner by measuring their conductance. We will examine how the conductivity of various solutions changes as the concentration and the identity of ions change. We will also see how conductivity can be used to follow chemical reactions.
Measuring Conductance The conductance of an electrolytic or electronic conductor is the reciprocal of its resistance in ohms. At one