Chemistry Chapter 10: Acids and Bases (4 Stars)

Question 1

______ acids dissociate to produce an excess of hydrogen ions in solution.. ______ bases dissociate to produce an excess of hydroxide ions in solution.

Answer 1

Arrhenius

Question 2

Brønsted–Lowry ____ are species that can donate hydrogen ions. Brønsted– Lowry _____ are species that can accept hydrogen ions.

Answer 2

acids

bases

Question 3

Lewis ____ are electron-pair acceptors. Lewis ____ are electron-pair donors.

Answer 3

acids

bases

Question 4

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).

Answer 4

Arrhenius

Question 5

______ species are those that can behave as an acid or base.

Answer 5

Amphoteric

Amphiprotic species are amphoteric species that specifically can behave as a Brønsted–Lowry acid or Brønsted–Lowry base.

Question 6

_____ 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.

Answer 6

Water

Question 7

______ species of polyvalent acids and bases can also behave as amphoteric and amphiprotic species.

Answer 7

Conjugate

Question 8

The water dissociation constant, Kw, is _____ at 298 K. Like other equilibrium constants, Kw is only affected by changes in temperature.

Answer 8

10–14

Question 9

pH and pOH can be calculated given the concentrations of _____ and OH– ions, respectively. In aqueous solutions, pH + pOH = 14 at 298 K.

Answer 9

H3O+

Question 10

_____ acids and bases completely dissociate in solution.

Answer 10

Strong

Question 11

Weak acids and bases do/ do not completely dissociate in solution and have corresponding dissociation constants (Ka and Kb, respectively).

Answer 11

do not

Question 12

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.

Answer 12

deprotonated.

Question 13

Strong acids and bases have very weak (inert) _______

Answer 13

conjugates.

Question 14

Weak acids and bases have _____ conjugates.

Answer 14

weak

Question 15

______ reactions form salts and (sometimes) water.

Answer 15

Neutralization

Question 16

A ______ is defined as one mole of the species of interest.

Answer 16

equivalent

Question 17

In acid–base chemistry, _____ is the concentration of acid or base equivalents in solution.

Answer 17

normality

Question 18

_____ 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

Answer 18

Polyvalent

Question 19

_____ are used to determine the concentration of a known reactant in a solution.

Answer 19

Titrations

Question 20

The titrant has a known ______ and is added slowly to the titrand to reach the equivalence point.

Answer 20

concentration

Question 21

The titrand has an unknown concentration but a known ______

Answer 21

volume.

Question 22

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.

Answer 22

half-equivalence point

Question 23

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.

Answer 23

steepest

Question 24

Strong acid and strong base titrations have equivalence points at pH ____

Answer 24

pH = 7.

Question 25

Weak acid and strong base titrations have equivalence points at pH ____.

Answer 25

pH > 7.

Question 26

Weak base and strong acid titrations have equivalence points at pH ____

Answer 26

pH < 7.

Question 27

Weak acid and weak base titrations can have equivalence points above or below 7, depending on the relative _____ of the acid and base.

Answer 27

strength

Question 28

_____ are weak acids or bases that display different colors in their protonated and deprotonated forms.

Answer 28

Indicators

Question 29

The indicator chosen for a titration should have a pKa close to the _____ of the expected equivalence point.

Answer 29

pH

Question 30

The _____ of a titration is when the indicator reaches its final color.

Answer 30

endpoint

Question 31

Multiple buffering regions and equivalence points are observed in ______ acid and base titrations.

Answer 31

polyvalent

Question 32

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.

Answer 32

salt

Question 33

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.

Answer 33

resist

Question 34

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.

Answer 34

pKb