acids + bases

Question 1

acid

Answer 1

proton doner

Question 2

base

Answer 2

proton acceptor

Question 3

acid-base reaction

Answer 3

transfer of a single proton from one species to another

Question 4

Kᵥᵥ

Answer 4

1) autoprotolysis constant
2) [H₃O⁺][OH⁻]
3) 1 x 10⁻¹⁴

Question 5

Why is pure water neutral?

Answer 5

equal concentrations of H₃O⁺ + OH⁻

Question 6

pH =

Answer 6

-log[H₃O⁺]

Question 7

[H₃O⁺] =

Answer 7

10⁻ᵖᴴ

Question 8

Kₐ

Answer 8

1) acidity constant

2) [H⁺][A⁻]/[HA]

Question 9

K₆

Answer 9

1) basicity constant

2) [BH⁺][OH⁻]/[B]

Question 10

pKₐ =

Answer 10

-log Kₐ

Question 11

pK₆ =

Answer 11

-log K₆

Question 12

The larger the Kₐ, the ? the acid

Answer 12

stronger

Question 13

The smaller the Kₐ, the ? the acid

Answer 13

stronger

Question 14

Kₐ K₆ =

Answer 14

Kᵥᵥ

Question 15

pKₐ + pK₆ =

Answer 15

pKᵥᵥ

Question 16

binary acid

Answer 16

acid containing H and only one other element, generally a non-metal

Question 17

Does acidity increase or decrease as we proceed down any group?

Answer 17

increase

Question 18

Why does acidity increase as we proceed down any group?

Answer 18

decreasing bond dissociation enthalpy

Question 19

oxoacid

Answer 19

acid composed of hydrogen, oxygen, + some other element

Question 20

What feature is common to all oxoacids?

Answer 20

O-H group bonded to some central atom

Question 21

buffer solution

Answer 21

contains appreciable amounts of both a weak acid/base + its conjugate base/acid

Question 22

What is the pH range over which a buffer is effective determined by?

Answer 22

pKₐ / pK₆ + ratio of conjugate pairs present in solution

Question 23

How can the pH of a buffer solution be calculated?

Answer 23

Henderson-Hasselbalch equation

Question 24

Henderson-Hasselbalch equation

Answer 24

1) pH = pKₐ + log ([A⁻]/[HA])

2) pH = pKₐ + log (nA⁻/nHA)

Question 25

When do buffer solutions work most efficiently?

Answer 25

when the ratio of [A⁻] to [HA] is close to 1

Question 26

When does pH = pKₐ?

Answer 26

when [A⁻] = [HA]

Question 27

buffer capacity

Answer 27

measure of how much H₃O⁺ + OH⁻ that can be added without causing a significant change in pH

Question 28

endpoint

Answer 28

pH at which the colour of the acid-base indicator changes

Question 29

equivalence point

Answer 29

pH at which the reaction stoichiometry is satisfied