Chemistry Chapter 10: Acids and Bases (4 Stars) Flashcards
______ acids dissociate to produce an excess of hydrogen ions in solution.. ______ bases dissociate to produce an excess of hydroxide ions in solution.
Arrhenius
Brønsted–Lowry ____ are species that can donate hydrogen ions. Brønsted– Lowry _____ are species that can accept hydrogen ions.
acids
bases
Lewis ____ are electron-pair acceptors. Lewis ____ are electron-pair donors.
acids
bases
All _____ acids and bases are Brønsted–Lowry acids and bases, and all Brønsted–Lowry acids and bases are Lewis acids and bases; however, the converse of these statements is not necessarily true (that is, not all Lewis acids and bases are Brønsted–Lowry acids and bases, and not all Brønsted–Lowry acids and bases are Arrhenius acids and bases).
Arrhenius
______ species are those that can behave as an acid or base.
Amphoteric
Amphiprotic species are amphoteric species that specifically can behave as a Brønsted–Lowry acid or Brønsted–Lowry base.
_____ is a classic example of an amphoteric, amphiprotic species—it can accept a hydrogen ion to become a hydronium ion, or it can donate a hydrogen ion to become a hydroxide ion.
Water
______ species of polyvalent acids and bases can also behave as amphoteric and amphiprotic species.
Conjugate
The water dissociation constant, Kw, is _____ at 298 K. Like other equilibrium constants, Kw is only affected by changes in temperature.
10–14
pH and pOH can be calculated given the concentrations of _____ and OH– ions, respectively. In aqueous solutions, pH + pOH = 14 at 298 K.
H3O+
_____ acids and bases completely dissociate in solution.
Strong
Weak acids and bases do/ do not completely dissociate in solution and have corresponding dissociation constants (Ka and Kb, respectively).
do not
In the Brønsted–Lowry definition, acids have conjugate bases that are formed when the acid is _______ Bases have conjugate acids that are formed when the base is protonated.
deprotonated.
Strong acids and bases have very weak (inert) _______
conjugates.
Weak acids and bases have _____ conjugates.
weak
______ reactions form salts and (sometimes) water.
Neutralization
A ______ is defined as one mole of the species of interest.
equivalent
In acid–base chemistry, _____ is the concentration of acid or base equivalents in solution.
normality
_____ acids and bases are those that can donate or accept multiple electrons. The normality of a solution containing a polyvalent species is the molarity of the acid or base times the number of protons it can donate or accept. Titration and Buffers
Polyvalent
_____ are used to determine the concentration of a known reactant in a solution.
Titrations
The titrant has a known ______ and is added slowly to the titrand to reach the equivalence point.
concentration
The titrand has an unknown concentration but a known ______
volume.
The _______ is the midpoint of the buffering region, in which half of the titrant has been protonated (or deprotonated); thus, [HA] = [A– ] and a buffer is formed.
half-equivalence point
The equivalence point is indicated by the ______ slope in a titration curve; it is reached when the number of acid equivalents in the original solution equals the number of base equivalents added, or vice-versa.
steepest
Strong acid and strong base titrations have equivalence points at pH ____
pH = 7.
Weak acid and strong base titrations have equivalence points at pH ____.
pH > 7.
Weak base and strong acid titrations have equivalence points at pH ____
pH < 7.
Weak acid and weak base titrations can have equivalence points above or below 7, depending on the relative _____ of the acid and base.
strength
_____ are weak acids or bases that display different colors in their protonated and deprotonated forms.
Indicators
The indicator chosen for a titration should have a pKa close to the _____ of the expected equivalence point.
pH
The _____ of a titration is when the indicator reaches its final color.
endpoint
Multiple buffering regions and equivalence points are observed in ______ acid and base titrations.
polyvalent
Buffer solutions consist of a mixture of a weak acid and its conjugate ____ or a weak base and its conjugate salt; they resist large fluctuations in pH.
salt
Buffering capacity refers to the ability of a buffer to ____ changes in pH; maximal buffering capacity is seen within 1 pH point of the pKa of the acid in the buffer solution.
resist
The Henderson–Hasselbalch equation quantifies the relationship between pH and pKa for weak acids and between pOH and ____ for weak bases; when a solution is optimally buffered, pH = pKa and pOH = pKb.
pKb
