 | Term | Definition |
| |
Arrhenius acid |
any substance that provides H+ ions when dissolved in water |
| |
Arrhenius base |
any substance that provides OH- ions when dissolved in water |
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Bronsted acid |
any hydrogen containing substance that is capable of donating a proton (H+) to another substance |
| |
Bronsted base |
any substance capable of accepting a proton from another substance |
| |
conjugate base |
species remaining when a Bronsted acid donates a proton |
| |
conjugate acid-base pair |
a Bronsted acid and its conjugate base |
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neutral |
term used to describe any water solution where the concentrations of H3O+ and OH- are equal; also a water solution with pH=7 |
| |
ion product of water |
equilibrium constant for the dissociation of pure water into H3O+ and OH- |
| |
acidic solution |
solution where the concentration of H3O+ is greater than the concentration of OH-; also a solution where the pH is less than 7 |
| |
basic or alkaline solution |
solution where the concentration of OH- is greater than the concentration of H3O+; also a solution where the pH is greater than 7 |
| |
pH |
negative logarithm of the molar concentration of H+ (H3O+) in a solution |
| |
activity series |
tabular representation of the tendencies of metals to react with H+ |
| |
neutralization reaction |
reaction where an acid and base react completely, leaving a solution that contains only a salt and water |
| |
salt |
solid crystalline ionic compound at room temperature that contains the cation of a base and the anion of an acid |
| |
cation |
+ charged ion |
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anion |
- charged ion |
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hydrate |
salt that contains specific numbers of water molecules as part of the solid crystalline structure |
| |
water of hydration |
water retained as part of the solid crystalline structure of some salts |
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equivalent of salt |
amount that will produce 1 mol of positive electrical charge when dissolved and dissociated |
| |
strong acids and strong bases |
acids and bases that dissociate (ionize) essentially completely when dissolved to form a solution |
| |
weak (or moderatly weak) acids and bases |
acids and bases that dissociate (ionize) less than completely when dissolved to form a solution |
| |
acid dissociation constant |
equilibrium constant for the dissociation of an acid |
| |
monoprotic acid |
acid that gives up only one proton (H+) per molecule when dissolved |
| |
diprotic acid |
an acid that gives up two protons (H+) per mole when dissolved |
| |
triprotic acid |
an acid that gives up three protons (H+) per molecule when dissolved |
| |
titration |
an analytical procedure where one solution (often a base) of known concentration is slowly added to a measured volume of an unknown solution (often an acid); the volume of the added solution is measured with a buret |
| |
equivalence point of a titration |
point where the unknown solution has exactly reacted with the known solution; neither is in excess |
| |
endpoint of titration |
point where the titration is stopped on the basis of an indicator color change or pH meter reading |
| |
hydrolysis reaction |
any reaction with water; for salts it is a reaction of the acidic cation and or basic anion of the salt with water |
| |
buffer |
solution with the ability to resist changing pH when acids (H+) or bases (OH-) are added |
| |
buffer capacity |
the amout of acid (H+) or base (OH-) that can be absorbed by a buffer without causing a significant change in pH |
| |
pKa |
negative logarithm of Ka |
| |
Henderson-Hasselbalch equation |
relationship between the pH of a buffer, pKa, and the concentrations of acid and salt in the buffer |
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