Chapter13:Acid and Bases

Kw

ion- product constant (or the dissociation constant for water)

Oxyacids

________- acidic proton is attached to an oxygen atom.

Vinegar

contains acetic acid and is used in salad dressings.

Arrhenius concept

acids produce hydrogen ions in aqueous solution, while bases produce hydroxide ions.

Conjugate base

everything that remains of the acid molecule after a proton is lost.

Salts

that consist of the cations of strong bases and the anions of strong acids have no effect on [H+] when dissolved in water.

Acid base equilibria

must focus on the solution components and their chemistry.

Common ion effect

shift in equilibrium position that occurs because of the addition of an ion already.

Amphoteric

can behave either as an acid or as a base.

amount of protons

Buffering capacity- ________ or hydroxide ions the buffer can absorb without a significant change in pH.

Acid strength

equilibrium position of its dissociation (ionization) reaction.

Lewis base

an electron- pair donor.

conjugate acid

Kb always refers to the reaction of a base with water to form the ________ and the hydroxide ion.

Organic acids

acids with a carbon atom backbone, commonly contain the carboxyl group.

Conjugate acid

formed when the proton is transferred to the base.

Arrhenius concept

acids produce hydrogen ions in aqueous solution, while bases produce hydroxide ions

Brønsted-Lowry model

an acid is a proton (H+) donor, and a base is a proton acceptor

conjugate base

everything that remains of the acid molecule after a proton is lost

conjugate acid

formed when the proton is transferred to the base

conjugate acid-base pair

two substances related to each other by the donating and accepting of a single proton

Ka

acid dissociation constant

Acid strength

equilibrium position of its dissociation(ionization) reaction

strong acid

equilibrium lies far to the right

weak acid

equilibrium lies far to the right

diprotic acid

acid having two acidic protons

oxyacids

acidic proton is attached to an oxygen atom

Organic acids

acids with a carbon atom backbone, commonly contain the carboxyl group

monoprotic acids

acid having one acidic protons

amphoteric

can behave either as an acid or as a base

Kw

ion-product constant (or the dissociation constant for water)

pH scale

represent solution acidity

acid-base equilibria

must focus on the solution components and their chemistry

triprotic acid

acid having three acidic protons

Lewis Acid-base model

An even more general model for acid-base behavior

Lewis acid

an electron-pair acceptor

Lewis base

an electron-pair donor

common ion effect

shift in equilibrium position that occurs because of the addition of an ion already

buffered solution

resists a change in its pH when either hydroxide ions or protons are added

buffering capacity

amount of protons or hydroxide ions the buffer can absorb without a significant change in pH