6 - Acids and Bases Flashcards
Arrhenius acid=
Arrhenius base=
Bronsted and Lowry acid=
Bronsted and Lowry base=
Lewis acid=
Lewis base=
pH =
Arrhenius acid= is anything that produces hydrogen ions in aqueous solution.
Arrhenius base= anything that produces hydroxide ions in aqueous solution.
Bronsted and Lowry acid= anything that donates a proton.
Bronsted and Lowry base= anything that accepts a proton.
Lewis acid= anything that accepts a pair of electrons.
Lewis base= anything that donates a pair of electrons.
pH = -log[H+]
Amphoteric=
*Acid taste _______, Bases taste ________
*Bases are _________ when wet
*Many reactions in living cells involve the transfer of a _______. The rate of such reactions depends upon the concentration of ____________
Amphoteric= substances that act as either an acid or base depending on their environment.
*Acid taste sour or tart, Bases taste bitter
*Bases are slippery when wet
*Many reactions in living cells involve the transfer of a proton. The rate of such reactions depends upon the concentration of H+ ions or the pH.
Polyprotic acids=
Diprotic acid=
*Assume that strong acids or bases completely _____ in water.
*in a series of oxyacids, more _______ means a stronger acids!
Polyprotic acids= acids that can donate more than one proton.
Diprotic acid= an acid that can donate two protons.
*Assume that strong acids or bases completely dissociate in water.
*in a series of oxyacids, more oxygens means a stronger acids!
Autoionization of water=
H2O + H2O –>
Kw =
Autoionization of water= pure water reacts with itself to form hydronium and hydroxide ions as follows:
H2O + H2O –> H3O+ + OH-
Kw = [H+][OH-]
Acid dissociation constant Ka=
Ka = (equation)
Kb=
Kb = (equation)
*a pKa less than _____ or a Ka greater than ____ indicates a strong base.
Acid dissociation constant Ka= an acid will have its own equilibrium constant in water.
Ka = [H+][A-]
[HA]
Kb= the equilibrium constant for the reaction of the conjugate base with water.
Kb = [OH-][HA]
[A-]
*a pKa less than zero or a Ka greater than 1 indicates a strong base.
Salts=
*When considering salts, remember all ____, except those of the ______act as weak lewis acids in aqueous solutions.
Salts= are ionic compounds that dissociate in water. They dissociate creating acidic or basic conditions.
*When considering salts, remember all cations, except those of the alkali metals and the heavier alkaline earth metals (Ca, Sr, and Ba) act as weak lewis acids in aqueous solutions.
Titration=
Titrant=
Titration= a drop by drop mixing of an acid and a base.
Titrant= titrations are performed in order to find the concentration of some unknown by comparing it with the concentration of the titrant.
Half equivalence point=
Buffered=
pH =
Half equivalence point= is the point where exactly one half of the acid has been neutralized by the base.
Buffered= the spot where we could add the largest amount of base or acid with the least amount of change in pH.
pH = pKa + log [A-]
[HA]
Indicator=
Buffer=
Indicator= is a chemical that can be used to find the eq. point; and it has two points of color change which give the range of an indicator. Endpoint is where the indicator changes color.
Buffer= is weak acid and its conjugate base. And pH = pKa
