General Chemistry Ch 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

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 accepts

Question 6

Lewis bases

Answer 6

Electron pair donors

Question 7

Arrhenius/Bronsted Lowry connection

Answer 7

All Arrhenius acids/bases are Bronsted-Lowry acid/bases but reverse not necessarily true

Question 8

Bronsted-Lowry/Lewis connection

Answer 8

All Bronsted-Lowry acids/bases are Lewis acids/bases but reverse not necessarily true

Question 9

Amphoteric species

Answer 9

Those that can behave as an acid or base, water good example, also conjugate species of polyvalent acids/bases

Question 10

Amphiportic species

Answer 10

Amphoteric species that specifically can behave as a Bronsted-Lowry acid or Bronsted-Lowry base, water good example, also conjugate species of polyvalent acids/bases

Question 11

Water dissociation constant

Answer 11

Kw = 10^-14 at 298 K, only affected by changes in temperature

Question 12

pH and pOH

Answer 12

Can be calculated given the concentrations of H3O+ and OH- ions, respectively, in aqueous solutions pH+pOH=14

Question 13

Strong acids/bases

Answer 13

Completely dissociate in solution, very weak/inert conjugates

Question 14

Weak acids/bases

Answer 14

Do not completely dissociate in solution and have corresponding dissociation constants (Ka and Kb respectively), weak conjugates

Question 15

Conjugate bases

Answer 15

Formed when a Bronsted-Lowry acid is deprotonated

Question 16

Conjugate acids

Answer 16

Formed when a Bronsted-Lowry base is protonated

Question 17

Neutralization reactions

Answer 17

Form salt and water

Question 18

Equivalent

Answer 18

One mole of the species of interest

Question 19

Normality

Answer 19

In acid base chemistry, the concentration of acid or base equivalents in solution

Question 20

Polyvalent

Answer 20

Acids and bases that can donate or accept multiple electrons, 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, multiple offering regions and equivalence points observed during titration

Question 21

Titrations

Answer 21

Used to determine the concentration of a known reactant in solution

Question 22

Titrant

Answer 22

Has a known concentration and is added slowly to the tetrad to reach the equivalence point during a titration

Question 23

Titrand

Answer 23

Has an unknown concentration but a known volume during a titration

Question 24

Half equivalence point

Answer 24

The midpoint of the buggering region, in which half of the titrant has been protonated or deprotonated, thus [HA] = [A-] and a buffer is formed

Question 25

Equivalence point

Answer 25

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 26

Strong acid and strong base titration

Answer 26

Equivalence point is around pH=7

Question 27

Weak acid and strong base titration

Answer 27

Equivalence point at pH>7

Question 28

Weak base and strong acid titration

Answer 28

Equivalence point at pH<7

Question 29

Weak acid and weak base titration

Answer 29

Can have equivalence points above or below 7 depending on the relative strength of the acid and base

Question 30

Indicators

Answer 30

Weak acids or bases that displace different colors in their protonated and deprotonated forms, the one chosen for titration should have a pKa close to the pH of the expected equivalence point, endpoint of a titration is when the indicator reaches its final color

Question 31

Buffer 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, maximal buffering capacity is seen within 1 pH point of the pKa of the acid in the buffer solution

Question 33

Henderson-Hasselbalch equation

Answer 33

Quantifies the relationship between pH and pKa for weak acids and between pOH and kPb for weak bases, when a solution is optimally buffered, pH=pKa and pOH=pKb