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Acids and Bases
Head-Royce School Lehman Honors Chemistry Acid/Base Test May 28, 2013
Terms in this set (33)
a compound that has a pH of less than seven; releases or donates hydrogen ions in solution or accepts an electron pair
a compound that has a pH of more than seven; releases hydroxide ions in solution, accepts hydrogen ions or releases an electron pair
H₃O⁺, the conjugate acid ion that is made during the self-ionization of water
OH⁻, the conjugate base ion that is made during the self-ionization of water
the compound that is produced when a substance accepts a hydrogen ion from an acid
the compound that is produced when a substance donates a hydrogen ion to a base
a compound that ionizes in solution (such as HCl or NaOH)
a compound that does not ionize in solution (such as CH₃COOH and NH₃)
a compound that completely ionizes in solution to produce lots of ions (such as HCl or NaOH)
a compound that does not ionize in solution and produces little ions, in equilibrium (such as such as CH₃COOH and NH₃)
able to be dissolved in a solute
insoluble (sparingly soluble)
unable or barely able to be dissolved in a solute
acids release hydrogen ions (H⁺) in solution; bases release hydroxide ions (OH⁻) in solution
acids donate hydrogen ions (H⁺); bases accept hydrogen ions (H⁺)
acids accept electron pairs; bases donate electron pairs
an ion that can act as both an acid and a base
a molecule that has multiple hydrogens
a solution with a pH of seven; a solution that has equal concentrations of hydrogen ions and hydroxide ions
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
a mixture of compounds that resist change in pH; an acid and its conjugate base or a base and its conjugate acid
a substance that changes color to indicate a change in the pH of a solution
a substance or multiple substances that turn different colors to indicate the range of pHs of a solution
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
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
the measure of how acidic or basic a solution is; the negative log of the concentration of hydrogen ions (H⁺)
the measure of how acidic or basic a solution is; the negative log of the concentration of hydroxide ions (OH⁻)
the value of the equilibrium constant for the self-ionization of water
the solubility product constant; the amount of solute that can dissolve in a given solvent
the equilibrium constant value for an acid
the equilibrium constant value for a base
"goes to completion"
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