General Chemistry Chapter 10: Acids and Bases

Question 1

Arrhenius acids

Answer 1

dissociate to produce an excess of hydrogen ions in solution

Question 2

Arrhenius bases

Answer 2

dissociate to produce an excess of hydroxide ions in solution

Question 3

Bronsted-lowry acids

Answer 3

are species that can donate hydrogen ions

Question 4

Bronsted-lowry bases

Answer 4

species that can accept hydrogen ions.

Question 5

Lewis acids

Answer 5

Electron pair acceptors

Question 6

Lewis bases

Answer 6

Electron pair donors

Question 7

Amphoteric species

Answer 7

those that can behave as an acid or base

Question 8

Amphiprotic species

Answer 8

are amphoteric species that specifically can behave as a Bronsted-Lowry acid or Bronsted-Lowry base

Question 9

What is the classic example of an amphoteric, amphiprotic species?

Answer 9

Water or conjugate species of polyvalent acids and bases

Question 10

Water dissociation constant (Kw)

Answer 10

10^-14 at 298 K. It is only affected by changes in temperature.

Question 11

pH and pOH

Answer 11

Can be calculated given the concentrations of H3O+ and OH- respectively . In aqueous solutions, pH + pOH = 14 at 298 K.

Question 12

in solution, strong acids and bases

Answer 12

completely dissociate

Question 13

In solution, weak acids and bases

Answer 13

do not completely dissociate in solution and have corresponding dissociation constants (Ka and Kb)

Question 14

The conjugates of strong acids and bases have ___ conjugates

Answer 14

weak

Question 15

Neutralization reactions form:

Answer 15

salts and sometimes water

Question 16

Equivalent

Answer 16

one mole of the species of interest

Question 17

Normality

Answer 17

concentration of acid or base equivalents in solution.

Question 18

Polyvalent acids and bases

Answer 18

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.

Question 19

Titrations

Answer 19

Used to determine the concentration of a known reactant in solution.

Question 20

Titrant

Answer 20

has a known concentration and is added slowly to the titrand to reach the equivalence point.

Question 21

Titrand

Answer 21

has an unknown concentration, but a known volume

Question 22

Half-equivalence point

Answer 22

midpoint of the buffering region in which half of the titrant has been protonated (or deprotonated); thus [HA] = [A-] and a buffer is formed.

Question 23

Equivalence point

Answer 23

indicated by the steepest 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.

Question 24

Strong acid/strong base titrations have equivalence points at

Answer 24

pH=7

Question 25

Weak acid/strong base titrations have equivalence points at

Answer 25

pH >7

Question 26

Weak base/strong acid titrations have equivalence points at:

Answer 26

above or below 7, depending on the relative strength of the acid and base.

Question 27

Indicators

Answer 27

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

Question 28

The indicator pH

Answer 28

should have a pKa close to the pH of the expected equivalence point

Question 29

endpoint of a titration

Answer 29

is when the indicator reaches its final color

Question 30

In polyvalent acid and base titrations

Answer 30

multiple buffering regions and equivalence points are observed

Question 31

Buffering solutions

Answer 31

consist of a mixture of a weak acid and its conjugate salt or a weak base and its conjugate salt. They resist large fluctuations in pH.

Question 32

Buffering capacity

Answer 32

refers to the ability of a buffer to resist changes in pH; minimal buffering capacity is seen within 1 pH point of the pKa of the acid in the buffering solution.

Question 33

Henderson-Hasselbalch

Answer 33

quantifies the relationship between pH and pKa for weak acids and between pOH and pKb for weak bases.

Question 34

When a solution is optimally buffered, pH = & pOH=

Answer 34

pH = pKa and pOH = pKb