acids and bases
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24 Terms
Dissociation
The process by which an ionic compound breaks apart into ions in solution.
Ionization
The reaction of a covalent compound with water to form ions.
Strong electrolyte
A substance that fully ionizes or dissociates in water.
Weak electrolyte
A substance that does not fully ionize or dissociate in water.
Hydronium ion (H3O+)
The ion formed when a water molecule combines with a hydrogen ion (H+).
Binary acid
An acid consisting of hydrogen and one other nonmetal element.
Oxyacid
An acid that contains hydrogen, oxygen, and another element.
Arrhenius acid
A substance that increases the concentration of hydrogen ions (H+) in water.
Arrhenius base
A substance that increases the concentration of hydroxide ions (OH-) in water.
Bronsted-Lowry acid
A substance that donates a proton (H+) in a reaction.
Bronsted-Lowry base
A substance that accepts a proton (H+) in a reaction.
Conjugate acid
The species formed when a base gains a proton.
Conjugate base
The species that remains when an acid donates a proton.
pH scale
A scale that measures the acidity or basicity of a solution, from 0 (very acidic) to 14 (very basic), with 7 being neutral.
Strong acid
An acid that completely ionizes in solution.
Weak acid
An acid that partially ionizes in solution.
Titration
A laboratory method of determining the concentration of a solute by reacting it with a standard solution.
Equivalence point
The point in a titration at which the amount of acid equals the amount of base.
End point
The point in a titration at which an indicator changes color, signaling that the equivalence point has been reached.
Net ionic equation
An equation that shows only the ions that participate in a reaction, omitting spectator ions.
Spectator ion
An ion that does not participate in a chemical reaction and is present in both the reactants and products.
Molarity (M)
A measure of concentration, defined as moles of solute per liter of solution.
pOH scale
A scale that measures the hydroxide ion concentration, related to pH by the equation pH + pOH = 14.
Hydroxide ion (OH-)
An ion formed when a base dissociates in water, contributing to the solution's basicity.