Acid-bases

Question 1

any species that dissolves in aqueous solution to produce H+ ions

Answer 1

arrhenius acid

Question 2

any species that dissolves in aqueous solution to produce OH ions

Answer 2

arrhenius base

Question 3

any species that acts as a proton donor

Answer 3

bronsted-lowry acid

Question 4

any species that acts as a proton acceptor

Answer 4

bronsted-lowry base

Question 5

any species that accepts a pair of electrons

Answer 5

lewis acid

Question 6

any species that donates a pair of electrons

Answer 6

lewis base

Question 7

the species that is the acid with one proton lost

Answer 7

conjugate base

Question 8

The species that is the base with one proton gained

Answer 8

conjugate acid

Question 9

The stronger the base or acid, the ___ its conjugate is, and the weaker the base or acid, the __ its conjugate is

Answer 9

weaker, stronger

Question 10

The definitions of acid-bases in order of most specific to general are ____, _____, and ___. Arrehenius definition is concerned with reactions that only occur in __ __. Bronsted-lowry and arrhenius definitions are concerned with __ __, and the lewis definition is concerned with ____ transfers. The ___ definition is the most common

Answer 10

arrhenius, bronsted-lowry, lewis, aqueous solutions, protons transfers, electron, bronsted-lowry

Question 11

The higher the concentration of ___ ions the lower the pH, this is given by the equation ____

Answer 11

H+, pH = -log[H+]

Question 12

The higher the concentration of ___ ions the lower the pOH. This is given by the equation ____

Answer 12

OH-, pOH = -log[OH]

Question 13

The pH and pOH are the -_ concentrations of protons and hydroxide ions. The sum of pH and pOH is always __ for a solution at room temperature

Answer 13

log, 14

Question 14

In a neutral solution, both the pOH and pH are ___. In an acidic solution, the pH is ___7, and the pOH is ___ than 7. In a basic solution the pH is ___7 and the pOH is ___ 7

Answer 14

7, <, >, >, <

Question 15

describes the extent ot which a particular substance dissociates into its ions

Answer 15

dissociation constants

Question 16

Ka is given by the equation:

Answer 16

ka = [H3O+][A-]/[HA]

Question 17

kb is given by the equation

Answer 17

kb = [HB][OH]/[B]

Question 18

The dissociation constant of water is defined as ____ and is ____ at 25°C. Because equal concentrations of __- and ___ dissociate from H2O, water has a __ pH and Kw = _______, or _______

Answer 18

kw, 1E-14, H+, OH-, neutral, [OH][H+], ka(kb)

Question 19

The __ the pka the stronger the acid and the ___ its ability to donate protons. It is equal to ___

Answer 19

lower, greater, -log(Ka)

Question 20

The lower the pkb, the __ the base and the greater its ability to ___ a proton. It is equal to ____

Answer 20

stronger, accept, -logkb

Question 21

A strong acid is one where the ka is ___ 1 and is dissociates completely in water to form ___

Answer 21

> , H+

Question 22

A strong base is one where kb ___ 1, and dissociates completely in water to form ______

Answer 22

> , OH-

Question 23

Binary acids include __ ___ like __, ___, __ and ____. THe larger the __ __ of the halide, the more acidic the compound, and the ___ the bond between them

Answer 23

hydrogen halides, HI, HBr, HCl, HF, atomic radius, weaker

Question 24

acids that contain oxygen are called ____. The more oxygen molecules there are, the more ____ the compound

Answer 24

oxoacids, acidic

Question 25

The strength of an acid ___ as the stability of its conjugate base ___

Answer 25

increases, increases

Question 26

For oxoacids that have the same number of oxygen atoms, the compound with the more ____ central atom will be a stronger acid. This is because the more electronegative atom will be more ___ when the acid loses a proton and acquires a ___ charge

Answer 26

electronegative, stable, negative

Question 27

when a strong acid reacts with a strong base to produce water

Answer 27

neutralization reaction

Question 28

Neutralization reactions go to ___ and the moles can be calculated using the equation ____

Answer 28

completion, M1V1 = M2V2

Question 29

1 mole of ___+ ions neutralizes 1 mole of ___- ions

Answer 29

H, OH

Question 30

The product of a neutralization reaction of acids and bases

Answer 30

salt

Question 31

A strong acid and a weak base react to form a __ ___. A weak acid and a strong base form a ___ ___

Answer 31

acidic salt, basic salt

Question 32

To determine whether a salt is acidic or basic, break the salt into its respective ___, then add ___ or ___. Whichever acid or base is stronger determines whether the salt is acidic or basic. If both are strong, the salt is __

Answer 32

ions, H, OH, neutral

Question 33

If the basic salt includes a group ___ or group __ metal cation, the cation is neutral

Answer 33

I, II,

Question 34

a solution that resists a change in pH when small amounts of acid or base are added to it

Answer 34

buffer

Question 35

A buffer is made of a __ acid and __ base. The buffer works best when the acid and base and ___ are equal in ___

Answer 35

weak, weak, conjugates, concentration

Question 36

Acidic buffers are made by combining a __ acid and a ____, in a ___ ratio. They can also be made with a weak acid and ___ base in a ___ ratio. They can also be made with a __ and a ___ acid in a __ ratio

Answer 36

weak, salt, 1:!, strong, 2:1, salt, strong, 2:1

Question 37

Assume ___% ionization of weak acids and bases, and ____% ionization of strong acids, bases and ___

Answer 37

0, 100, salts

Question 38

to make alkaline buffers you can combine a ___ base and a ___ in a 1:1 ratio. You can also use a ____ base and ___ acid in a 2:1 ratio. You can also use a __ and a strong base in a ___ ratio

Answer 38

weak, salt, weak, strong, salt, 2:1

Question 39

The henderson-hasselbalch equation can be used to calculate the pH or pOH of a buffer and is given by ____.

Answer 39

pH = pka + log[A]/[HA]

Question 40

A buffer is considered to be a buffer if it is _____ of the ___

Answer 40

+/-1. pka

Question 41

___ is an experiment used to determine the unknown concentration of an acid or base by adding an acid or base of a __ __

Answer 41

titration, known concentration

Question 42

the solution of unknown concentration

Answer 42

analyte

Question 43

changes colour at the equivalence point

Answer 43

indicator

Question 44

the solution of known concentration

Answer 44

titrant

Question 45

The point at which the analyte has equal concentrations of OH and H; the point at which the amount of titrant added is just enough to neutralize the analyte solution

Answer 45

equivalence point

Question 46

Indicators are ___ acids or base that are used to estimate the __ __ of an acid-base titration. You should pick one with a ___ close to the __ of the equivalence

Answer 46

weak, equivalence point, pka, pH

Question 47

The ____ ____ point is seen when strong acids and weak bases are combined or when weak acids and strong bases are combined. It is the ___ of the __ ___, and is where ___

Answer 47

half equivalence point, midpoint, buffering region, pH = pKa

Question 48

The volume of analyte needed to reach the equivalence point is given by the equation ____

Answer 48

N1V1 = N2V2

Question 49

If a strong acid and base are added together, it should completely neutralize and the equivalence point should be a ___. If a strong acid and weak base are added, the equivalence point is ___ 7. If a weak acid and strong base are added the equivalence point is __7

Answer 49

7, <, >

Question 50

____ acids and bases can donate or accept more than 1 H+ ion. These titration curves usually feature multiple __ __ and multiple __ __

Answer 50

polyvalent, buffering regions, equivalence points