Which of these compounds are electrolytes? Consider each...

Which of these compounds are electrolytes? Consider each substance to be mixed with water.
(a) $\mathrm{NaHCO}_3$ (baking soda)
(b) $\mathrm{N}_2$ (insoluble gas)
(c) $\mathrm{AgNO}_3$
(d) HCOOH (formic acid)
(e) RbOH
(f) $\mathrm{K}_2 \mathrm{CrO}_4$

Key Concepts

Weak Electrolytes

Weak electrolytes are substances that only partially ionize in water, meaning that only a fraction of their molecules break into ions. This incomplete ionization results in a lower concentration of free ions in the solution, thus reducing their ability to conduct electricity.

Strong Electrolytes

Strong electrolytes are compounds, typically ionic in nature, that completely ionize in aqueous solution. This full dissociation results in a high concentration of ions, leading to effective electrical conductivity. Examples include many soluble salts and strong acids or bases.

Solubility in Water

Solubility is the ability of a substance to dissolve in water. For a compound to function as an electrolyte, it must be sufficiently soluble to release its constituent ions into the solution. Insoluble substances do not provide ions, and thus do not contribute to electrical conductivity in water.

Electrolytes

Electrolytes are substances that, when dissolved in water, produce a solution that can conduct electricity through the presence of mobile ions. This essential property is due to the dissociation of these compounds into their respective ions.

Dissociation and Ionization

Dissociation, or ionization, refers to the process by which compounds break into ions when dissolved in water. The extent of this process defines whether a substance acts as a strong electrolyte (completely dissociating) or a weak electrolyte (partially dissociating).

Transcript

Please give Ace some feedback