Chapter 19 - Acids, Bases, and Salts Flashcards
monoprotic acid
Acids that contain one ionizable hydrogen (ie diprotic acids = acids that have two ionizable hydrogens ext.)
conjugate acid
the particle formed when a base gains a hydrogen ion
conjugate base
is the particle that is left when a base donates a hydrogen ion
conjugate acid-base pair
is when two substances are related by the loss or gain of a single hydrogen ion
Hydronium ion
when a water molecule gains an extra hydrogen ion (H3O)
amphoteric
a substance that will either accept a hydrogen ion or donate it (an example is water)
Lewis acid
a substance that accepts a pair of electrons to form a covalent bond
Lewis base
a substance that donates a pair of electrons to form a covalent bond
self ionization
when water molecules produce ions
neutral solution
any aqueous solution that the hydrogen ions match the hydroxide ions
ion product constant for water
h+ x oh- = 1 x 10^-14
acidic solution
when the hydrogen ions outnumber the oh- ions
basic solution
when the oh- ions outnumber the h+ ions
alkaline solution
a basic solution
ph
the negative logarithm of the hydrogen ion concentration of a solution (ph=-log(H+)
strong acids
completely ionize in aqueous solutions
weak acids
ionize slightly in aqueous solutions
acid dissociation constant
is the ratio of the concentration of the dissociated form an acid to the concentration of the non ionized form
strong bases
completely break into metal ions and hydroxide ions aqueous solutions
weak bases
react with aqueous solutions to form the hydroxide ion and the conjugate acid of the base
base dissociation constant
is the ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the base.
neutralization reaction
when an acid and a base react in an aqueous solution to produce a salt and water
equivalence proportion
when the -oh ions match the h+ ions
titration
when you know one concentration and you use it to find another concentration
standard solution
the solution of the known concentration
end point
when the indicator changes color
salt hydrolysis
the cations of anions of a dissociated salt remove hydrogen ions or donate them to to the water
buffer
is a solution in which the ph remains relatively constant when small amounts of acids and bases are added
buffer capacity
the amount of acid or base that can be added to the buffer solution before a significant change in ph occurs.