| A | B |
|---|
| hydrolyzing salts | compounds derived from the reaction of a strong base with a weak acid or a strong acid with a weak base or a solution of a weak base and one of its salts |
| neutral | term used to describe the pH of a solution that results when one equivalent of a strong acid is mixed with one equivalent of a strong base |
| equivalence point | the number of moles of hydrogen ions equals the number of moles of hydroxide ions in a titration |
| buffer | solution that consists of a weak acid and one of its salts |
| acid dissociation constant | Ka = ([H+][A-])/[HA] |
| acidic solution | [H+] greater than [OH-] |
| salt hydrolysis | The cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water |
| alkaline (base) solution | [OH-] greater than [H+] |
| endpoint | point of neutralization as indicated by a color change in a titration |
| ion-product constant for water | Kw = [H+][OH-] = 1 x 10^-14 |
| neutral solution | [OH-] and [H+] = 1 X 10^-7 |
| amphoteric | describes a substance that can act as both an acid and a base |
| conjugate acid-base pair | two substances that are related by the loss or gain of a single hydrogen ion |
| hydronium ion | H3O+ |
| base dissociation constant | Kb = ([conjugate acid][OH-])/[base] |
| buffer capacity | the amount of acid or base that can be added to a buffer before a significant change in pH occurs |
| conjugate acid | particle formed when a base gains a hydrogen ion |
| conjugate base | particle remaining when an acid donates a hydrogen ion |
| diprotic acid | acids containing two ionizable hydrogens |
| Lewis acid | substance that accepts a pair of electrons in a reaction |
| Lewis base | substance that donates a pair of electrons in a reaction |
| Arrhenius acid | substances that release hydrogen ions (H+) in aqueous solution |
| Arrhenius base | substances the release hydroxide ions (OH-) in aqueous solution |
| Brönsted-Lowry acid | substance that is a hydrogen ion donor |
| Brönsted-Lowry base | substance that is a hydrogen ion acceptor |
| monoprotic acid | acids containing one ionizable hydrogen |
| neutralization reaction | reactions in which an acid and a base react to produce a salt and water |
| pOH | -log[OH-] |
| pH | -log[H+] |
| pH values between 0 and 7 | represent acidic solutions |
| pH values between 7 and 14 | represent alkaline (basic) solutions |
| pH value equal to 7 | represents a neutral solution |
| acid-base indicators | chemicals that change color in different ranges of pH values |
| salt hydolysis | the cations or anions of a dissociated salt remove or donate hydrogent ions to water |
| self-ionization | the reaction in which water molecules produce ions H2O(l) -> H+(aq) + OH-(aq) |
| standard solution | the solution of known concentration in a titration |
| strong acid | are completely ionized to release H+ ions in aqueous solution, have larger Ka values |
| strong base | are completely ionized to release OH- ions in aqueous solution, have larger Kb values |
| titration | process of adding a known amount of a solution of known concentration to determine the concentration of another solution |
| triprotic acid | acids containing three ionizable hydrogenss |
| weak acid | ionizes only slightly in aqueous solution to release H+ ions, have small Ka values |
| weak base | ionizes only slightly in aqueous solution to release OH- ions, have small Kb values |
