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DAT booster Chemistry > Acid-bases > Flashcards

Acid-bases Flashcards

1
Q

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

A

arrhenius acid

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2
Q

any species that dissolves in aqueous solution to produce OH ions

A

arrhenius base

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3
Q

any species that acts as a proton donor

A

bronsted-lowry acid

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4
Q

any species that acts as a proton acceptor

A

bronsted-lowry base

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5
Q

any species that accepts a pair of electrons

A

lewis acid

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6
Q

any species that donates a pair of electrons

A

lewis base

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7
Q

the species that is the acid with one proton lost

A

conjugate base

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8
Q

The species that is the base with one proton gained

A

conjugate acid

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9
Q

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

A

weaker, stronger

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10
Q

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

A

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

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11
Q

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

A

H+, pH = -log[H+]

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12
Q

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

A

OH-, pOH = -log[OH]

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13
Q

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

A

log, 14

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14
Q

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

A

7, <, >, >, <

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15
Q

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

A

dissociation constants

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16
Q

Ka is given by the equation:

A

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

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17
Q

kb is given by the equation

A

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

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18
Q

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 _______

A

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

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19
Q

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

A

lower, greater, -log(Ka)

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20
Q

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

A

stronger, accept, -logkb

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21
Q

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

A

> , H+

22
Q

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

A

> , OH-

23
Q

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

A

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

24
Q

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

A

oxoacids, acidic

25
Q

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

A

increases, increases

26
Q

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

A

electronegative, stable, negative

27
Q

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

A

neutralization reaction

28
Q

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

A

completion, M1V1 = M2V2

29
Q

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

A

H, OH

30
Q

The product of a neutralization reaction of acids and bases

A

salt

31
Q

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

A

acidic salt, basic salt

32
Q

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 __

A

ions, H, OH, neutral

33
Q

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

A

I, II,

34
Q

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

A

buffer

35
Q

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

A

weak, weak, conjugates, concentration

36
Q

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

A

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

37
Q

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

A

0, 100, salts

38
Q

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

A

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

39
Q

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

A

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

40
Q

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

A

+/-1. pka

41
Q

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

A

titration, known concentration

42
Q

the solution of unknown concentration

A

analyte

43
Q

changes colour at the equivalence point

A

indicator

44
Q

the solution of known concentration

A

titrant

45
Q

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

A

equivalence point

46
Q

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

A

weak, equivalence point, pka, pH

47
Q

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 ___

A

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

48
Q

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

A

N1V1 = N2V2

49
Q

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

A

7, <, >

50
Q

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

A

polyvalent, buffering regions, equivalence points

DAT booster Chemistry (13 decks)

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