1.5 Acid-Base Equilibria Flashcards
acid + metal ->
salt + hydrogen
acid + base ->
salt + water
acid + alkali ->
salt + water
acid + carbonate ->
salt + water + carbon dioxide
define Brønsted-Lowry acid
a proton (H+) donor
define Brønsted-Lowry base
a proton (H+) acceptor
What is a monobasic acid?
donates one proton per molecule
Name a dibasic acid
H2SO4
Name a tribasic acid
H3PO4
How does an acid relate to its conjugate base?
The acid has one more hydrogen ion than its conjugate base
How does a base relate to its conjugate acid?
The base has one less hydrogen ion than its conjugate acid
What is the conjugate base for HCl?
Cl^-
What is the conjugate acid for H2O?
H3O^+
What is the acid for the conjugate base NO3^-?
HNO3
What is the base for the conjugate acid H2SO4?
HSO4^-
What is an acid-base pair?
a pair of two species that transform into each other by gain or loss of a proton
What will a H+ ion do in an aqueous solution?
In an aqueous solution a H+ ion is too small to exist on its own and therefore will combine with H2O to form H3O+ ion (hydroxonium ion).
What does the pH of a solution depend on?
the concentration of H^+(aq)
How can pH be calculated?
pH = -log10[H+]
How can [H+] be calculated?
[H+] = 10^-pH
Name the transformation of a log equation used in the pH equation
logaB = C -> a^c = B
What is the relationship between pH and [H^+(aq)]
negative - low pH means a high [H^+(aq)]
Describe the strength of an acid HA
the extent of its dissociation into H^+ and A^- ions
What is a strong acid?
An acid that completely dissociates in solution