Classify each of the following aqueous solutions as a...

Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) $\mathrm{PbCl}_{2}$, (b) $\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}$ (c) $\mathrm{CsOH}$, (d) $\mathrm{H}_{2} \mathrm{~S},$ (e) $\mathrm{CrCl}_{2}$ (f) $\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}$

Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) $\mathrm{PbCl}_{2}$,
(b) $\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}$
(c) $\mathrm{CsOH}$,
(d) $\mathrm{H}_{2} \mathrm{~S},$
(e) $\mathrm{CrCl}_{2}$
(f) $\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}$

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Key Concepts

Electrolytes

Electrolytes are substances that dissolve in water to produce ions, which allow the solution to conduct electricity. Their behavior in solution—whether they dissociate completely or partially—directly affects their conductivity.

Strong Electrolytes

Strong electrolytes are compounds that completely or nearly completely ionize in aqueous solution, resulting in a high concentration of ions. This complete dissociation leads to excellent electrical conductivity.

Weak Electrolytes

Weak electrolytes only partially ionize or dissociate in water, which means that only a fraction of the dissolved molecules break into ions. As a result, their solutions conduct electricity but to a much lesser extent compared to strong electrolytes.

Nonelectrolytes

Nonelectrolytes are substances that do not produce any ions when dissolved in water, usually because they are covalent compounds. Since there are no ions in solution, nonelectrolytes do not conduct electricity.

Degree of Dissociation

The degree of dissociation refers to the fraction of a solute that breaks apart into ions in solution. It is a key factor in determining whether a substance acts as a strong or weak electrolyte, thereby influencing the solution's electrical conductivity.

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