Upgrade to remove ads
Only $35.99/year

Acid/Base Vocabulary

Terms in this set (33)

acid
a compound that has a pH of less than seven; releases or donates hydrogen ions in solution or accepts an electron pair
base
a compound that has a pH of more than seven; releases hydroxide ions in solution, accepts hydrogen ions or releases an electron pair
hydronium ion
H₃O⁺, the conjugate acid ion that is made during the self-ionization of water
hydroxide ion
OH⁻, the conjugate base ion that is made during the self-ionization of water
conjugate acid
the compound that is produced when a substance accepts a hydrogen ion from an acid
conjugate base
the compound that is produced when a substance donates a hydrogen ion to a base
strong electrolyte
a compound that ionizes in solution (such as HCl or NaOH)
weak electrolyte
a compound that does not ionize in solution (such as CH₃COOH and NH₃)
strong acid/base
a compound that completely ionizes in solution to produce lots of ions (such as HCl or NaOH)
weak acid/base
a compound that does not ionize in solution and produces little ions, in equilibrium (such as such as CH₃COOH and NH₃)
soluble
able to be dissolved in a solute
insoluble (sparingly soluble)
unable or barely able to be dissolved in a solute
Arrhenius model
acids release hydrogen ions (H⁺) in solution; bases release hydroxide ions (OH⁻) in solution
Brønsted-Lowry model
acids donate hydrogen ions (H⁺); bases accept hydrogen ions (H⁺)
Lewis model
acids accept electron pairs; bases donate electron pairs
amphoteric ion
an ion that can act as both an acid and a base
amphiprotic molecule
a molecule that has multiple hydrogens
neutral
a solution with a pH of seven; a solution that has equal concentrations of hydrogen ions and hydroxide ions
neutralization
a chemical reaction between an acid and a base that produces water and a salt
common ion effect
the lowering of the solubility of a compound if the solute shares a common ion with the solvent
buffer
a mixture of compounds that resist change in pH; an acid and its conjugate base or a base and its conjugate acid
indicator
a substance that changes color to indicate a change in the pH of a solution
universal indicator
a substance or multiple substances that turn different colors to indicate the range of pHs of a solution
titration
a process where the volume of two substances are measured very carefully in order to determine the concentration of one of the substances, assuming the other concentration is known;also used to determine the volume of a solution needed to completely react with a certain mass or volume of a sample
standard solution
a solution that has a known concentration; used to determine the concentration of other solutions
equivalence point (endpoint)
the stoichiometric point where there are an equal moles of acid and base in the solution
pH
the measure of how acidic or basic a solution is; the negative log of the concentration of hydrogen ions (H⁺)
pOH
the measure of how acidic or basic a solution is; the negative log of the concentration of hydroxide ions (OH⁻)
Kw
the value of the equilibrium constant for the self-ionization of water
Ksp
the solubility product constant; the amount of solute that can dissolve in a given solvent
Ka
the equilibrium constant value for an acid
Kb
the equilibrium constant value for a base
"goes to completion"
fully ionizes
Recommended textbook explanations

Modern Chemistry

1st EditionSarquis, J., Sarquis, M.
2,184 explanations

Foundations of Physical Science (Florida Edition)

3rd EditionTom C. Hsu
1,687 explanations

Physical Science

2nd EditionMcLaughlin, Thompson, Zike
1,490 explanations

Chemistry Matter and Change

1st EditionMcGraw-Hill
4,862 explanations