Definition Example The reason the example fits the definition
Acid
Base
Strong Electrolyte
Weak Electrolyte
Non-Electrolyte
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Acid
Definition: A substance that donates a proton (H+) in a solution.
Example: Hydrochloric acid (HCl)
Reason: When HCl is dissolved in water, it donates a proton (H+) to form hydronium ions (H3O+), thus acting as an acid.
Base
Definition: A substance that accepts a proton (H+) in a solution.
Example: Sodium hydroxide (NaOH)
Reason: When NaOH is dissolved in water, it accepts a proton (H+) from water to form hydroxide ions (OH-), thus acting as a base.
Strong Electrolyte
Definition: A substance that completely dissociates into ions in a solution, thus conducting electricity very well.
Example: Sodium chloride (NaCl)
Reason: When NaCl is dissolved in water, it completely dissociates into sodium ions (Na+) and chloride ions (Cl-), which can move freely and conduct electricity, making it a strong electrolyte.
Weak Electrolyte
Definition: A substance that partially dissociates into ions in a solution, thus conducting electricity poorly.
Example: Acetic acid (CH3COOH)
Reason: When acetic acid is dissolved in water, it only partially dissociates into ions, producing fewer ions that can conduct electricity, making it a weak electrolyte.
Non-Electrolyte
Definition: A substance that does not dissociate into ions in a solution, thus not conducting electricity.
Example: Sugar (C12H22O11)
Reason: When sugar is dissolved in water, it does not dissociate into ions. Therefore, it does not conduct electricity, making it a non-electrolyte.
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