Question | Answer |
Arrhenius acid | a compound that contains hydrogen and releases hydrogen cations (H+) in water |
Arrhenius base | a compound that contains hydroxide and releases hydrogen anions (OH-) in water |
Bronsted-Lowry acid | a substance that is a proton donor (H+) |
Bronsted-Lowry base | a substance that can accept protons (H+) |
monoprotic acid | an acid that contains only one ionizable hydrogen atom |
polyprotic acid | an acid that contains two or more ionizable hydrogen atoms |
pH | the negative logarithm of the concentration of H+ in a solution used to measure acidity and alkalinity |
pOH | the negative logarithm of the concentration of OH- in a solution |
strong acid | an acid that ionizes completely in a solution |
strong base | a base that ionizes completely in water |
weak acid | an acid that releases few hydrogen ions in a solution (ionizes slightly) |
weak base | a base that releases few hydrogen ions in a solution (ionizes slightly) |
conjugate acid | an acid that forms after a base gains a proton |
conjugate base | a base that forms after an acid loses an electron |
amphoteric | describes a substance such as water that has the properties of an acid and a base |
Kw | self-ionization constant of water |
neutral | solution that contains equal concentrations of hydronium ions and hydroxide ions |
indicator | a compound that can reversibly change colors depending on pH of the solution. |
neutralization reaction | when acids and bases come together to form water |
equivalence point | the point when two solutions used in a titration are present in equal amounts |
titration | a method used to determine the concentration of a substance by adding a solution of known volume |
buffer solution | a solution with resists change in pH/ changes pH very slightly/ keeps pH constant when small amounts of acid or base are added |
end point | occurs in a titration when the indicator changes color |