CHEM - Acids And Bases Flashcards
This definition of an acid is a slight modification of the original _____ definition, which was that an acid produces H+ in aqueous solution.
Arrhenius
an acid produces __in aqueous solution
H+
A substance that produces H3O+ ions in aqueous solution.
Acid
A substance that produces OH– ions in aqueous solution.
Base
One that reacts completely with water to form H3O+ ions.
Strong acid
One that reacts completely with water to form OH– ions.
Strong base
A substance that dissociates only partially in water to produce H3O+ ions.
Weak acid
A substance that only partially reacts with water to produce OH– ions.
Weak base
A proton donor.
Acid
A proton acceptor.
Base
A proton-transfer reaction.
Acid base reaction
Any pair of molecules or ions that can be interconverted by transfer of a proton.
Conjugate acid base pair
definitions do not require water as a reactant.
Brønsted–Lowry
An acid can be positively charged, neutral, or negatively charged; examples of each type are
H3O+, H2CO3, and H2PO4–.
A base can be negatively charged or neutral; examples are
OH–, Cl–, and NH3.
Acids are classified as ____ depending on the number of protons each may give up; examples are HCl, H2CO3, and H3PO4.
monoprotic, diprotic, or triprotic
A substance that can act as either an acid or a base is said to be
amphiprotic
The product of [H3O+] and [OH–] in any aqueous solution is equal to
1.0 x 10–14.
One whose pH is less than 7.0.
Acidic solution
One whose pH is equal to 7.0.
Neutral solution
One whose pH is greater than 7.0.
Basic solution
The ion product of water, K , is
1.0 x 10–14
A solution that resists change in pH when limited amounts of acid or base are added to it.
PH buffer
A pH buffer is an acid or base
“shock absorber.”
The amount of hydronium or hydroxide ions that a buffer can absorb without a significant change in pH.
Buffer capacity
H2CO3 and its conjugate base, HCO3–
Carbonate buffer
H2PO4– and its conjugate base, HPO42–
Phosphate buffer
A mathematical relationship between:
• pH
• pKa of the weak acid, HA
• The concentrations of HA and its conjugate base A–.
Henderson–Hasselbalch equation
