Rank the conductivities of 1 M aqueous solutions of each of...

Rank the conductivities of $1 M$ aqueous solutions of each of the following solutes, starting with the most conductive:
(a) acetic acid; (b) methanol; (c) sucrose (table sugar);
(d) hydrochloric acid.

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Key Concepts

Electrolytes

Electrolytes are substances that dissolve in water to produce ions, which are responsible for conducting electricity in solution. Understanding electrolytes is fundamental to predicting and comparing the conductivities of solutions because the presence and mobility of ions dictate the solution's electrical conductivity.

Strong and Weak Electrolytes

The distinction between strong and weak electrolytes is crucial, as strong electrolytes dissociate completely into ions in solution, resulting in high conductivity, whereas weak electrolytes dissociate only partially and thereby produce fewer ions. This concept helps explain why some aqueous solutions conduct electricity better than others.

Nonelectrolytes

Nonelectrolytes are compounds that do not generate ions when dissolved in water. Their lack of ion production means they contribute little to no electrical conductivity, which is important when comparing substances like certain organic compounds that behave as nonelectrolytes.

Degree of Dissociation and Ion Mobility

The degree of dissociation refers to the fraction of a solute that ionizes in solution. This, combined with the mobility of the resulting ions, determines the overall conductivity of the solution. A higher degree of ionization leads to more charge carriers and, thus, a higher conductivity.

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