Arrhenius definition
an acid is a substance that produces hydrogen ions (H+) in solution, and a base is a substance that produces hydroxide (OH-) ions in solution
hydronium ion
H3O+, a water molecule with a bond to a proton, produced when an acid is added to water
Bronsted-Lowry definition
defines an acid as a proton donor and a base as a proton acceptor
conjugate base
the product formed when an acid loses a proton
conjugate acid
the product formed when a base accepts a proton, H+, neutral or positively charged
amphoteric molecule
water: it can act as both an acid and a base
strong acids
inorganic compounds that include HCl, HBr, HI, HNO3, H2SO4, and HClO4
strong bases
ionic compounds that contain hydroxide ions and groups 1A or 2A metal cation
conjugate acid-base pairs
one pair is always water and hydroxide ion or water and hydronium ion; differs by a hydrogen ion
weak acid
dissociates to a small extent in solution. At equilibrium there is a mixture of mainly the un-ionized acid, a small amount of its conjugate base, and hydronium ions
weak acids
include carboxylic acids, carbonic acid, phosphoric acid, organic derivatives of phosphoric acid, and the conjugate acids of amines
weak base
ionizes to a small extent in solution. At equilibrium there is a mixture of mainly the un-ionized base, a small amount of its conjugate acid, and hydroxide ions
weak bases
include ammonia, amines, hydrogen carbonate ion, carbonate ion, and the conjugate base of carboxylic acids
Le Chatelier's principle
allows one to predict how the equilibrium reaction for a weak acid of a weak base will shift if a reactant or product is added or removed. The equilibrium shifts in the direction that restores equilibrium
pH
a quantitative measure of the hydronium ion concentration in solution
acidic solution
pH less than 7
basic solution
pH greater than 7
neutral solution
pH equal to 7
autoionization of water
a reversible reaction that occurs in pure water between two water molecules to produce a hydroxide ion and a hydronium ion
physiological pH
the pH of arterial blood: pH= 7.35-7.45
neutralization reaction
the chemical reaction between an acid and a base to form a neutral compound like water and a salt, or water, a salt, and CO2
buffer
a solution that resists changes in pH upon addition of a small amount of acid or base; weak acid and its conjugate base, or a weak base and its conjugate acid
buffer capacity
the amount of acid or base that can be added to a buffer and still maintain the pH; directly related t the amount of buffer components in a solution
acidosis
pH below 7.35
alkalosis
pH above 7.45
acid
according to the Arrhenius definition, a substance that produces hydrogen ions, H+, in solution. According to the Bronsted-Lowry definition, a proton donor
acid-base homeostasis
maintenance of the proper pH balance in the blood and other bodily fluids
Acid Dissociation Constant, Ka
the product of the concentration of products divided by the concentration of reactants for the reaction of an acid with water at equilibrium
alkaline
a solution with a pH greater than 7; a basic solution
base
according to the Arrhenius definition, a substance that produces hydroxide ions, OH-, in solution. According to the Bronsted-Lowry definition, a proton acceptor
homeostasis
a balanced system
metabolic acidosis
a medical condition resulting when blood pH falls below normal as a result of metabolic disorder
metabolic alkalosis
a medical condition resulting when blood pH rises above normal as a result of metabolic disorder
net reaction
represents the actual species reacting in a neutralization reaction. For example: H+ + OH-= H2O
pH indicator paper
special dye-coated papers that can be used to determine the approximate pH of a solution by a visible color change
respiratory acidosis
a condition in which blood pH falls below normal as a result of weak breathing and ineffective removal of CO2 from the blood
respiratory alkalosis
a condition in which blood pH rises above normal because CO2 is eliminated too quickly as result of hyperventilating or breathing too fast
spectator ions
an ion dissolved in solution that is not involved in the chemical reaction
strong acid
an acid that is fully dissociated in water
strong base
a base that is fully dissociated in water such as hydroxide ion - containing salts of group 1A or 2A metal cations
amines
weak base, reacts with an acid to form a salt composed of the conjugate acid of the amine and the conjugate base of the acid; salts are soluble in water because they are neutral
carboxylic acids
common organic acids