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ap chemistry > Unit 8 - Acids and Bases > Flashcards

Unit 8 - Acids and Bases Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

What is the balanced chemical equation of autoionization of water?

A

2H2O H3O+ + OH-

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2
Q

What is the equilibrium constant of pure water at 25 degrees Celsius?

A

1 * 10^-14

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3
Q

Kw is equivalent to…

A

[H3O+][OH-]

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4
Q

The “p” in pH means…

A

to take the -LOG of the measurements that follow

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5
Q

In acidic solutions, ….

A

[H3O+] > [OH-]

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6
Q

In basic solutions, ….

A

[H3O+] < [OH-]

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7
Q

In neutral solutions, ….

A

[H3O+] = [OH-]

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8
Q

The pH scale measures …

A

the relative concentrations of H3O+ and OH-

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9
Q

As the concentration of H3O+ increases, the pH

A

decreases

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10
Q

What is the chemical formula for hydroxide ion?

A

OH-

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11
Q

What is the chemical formula for hydronium ion?

A

H3O+

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12
Q

In a pH of 7.345, the “7” represents …

A

the magnitude

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13
Q

In a pH of 7.345, the “345” represents ….

A

the measurement

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14
Q

From [H3O+] to pH …

A

[H3O+] = 10 ^ -pH

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15
Q

From pH to [H3O+] …

A

pH = -log [H3O+]

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16
Q

From [OH-] to pOH …

A

[OH-] = 10^-pOH

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17
Q

From pOH to [OH-] …

A

pOH = -log [OH-]

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18
Q

At 25 degrees Celsius, 14 is equivalent to…

A

pH + pOH

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19
Q

At 25 degrees Celsius, 1 * 10^-14 is equivalent to

A

[H3O+][OH-]

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20
Q

Pkw at 25 degrees Celsius is …

A

14

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21
Q

If [H3O+] has a coefficient of 1, then the pH is …

A

absolute value of the exponent.

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22
Q

If [H3O+] has a coefficient other than 1, then the pH is…

A

absolute value of the exponent minus one

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23
Q

The autoionization of water is an _________ process.

A

ENDOTHERMIC

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24
Q

As the temperature increases, the equilibrium constant will ….

A

Increase as well.

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25
Q

Kw increases with temperature because …

A

reaction shifts to form products and consume reactants

Products = [H3O+][OH-}

26
Q

In pure water how does the concentration of OH- and H3O+ compare?

A

In PURE WATER [OH-} is EQUAL to {H3O+]

27
Q

Kw is equal to….

A

10 ^ -pKW

28
Q

pKw is equal to …

A

-log [Kw]

29
Q

As temperature increase , the pH of pure water …

A

Decreases

30
Q

How do we determine whether a solution is acidic, basic, or neutral at temperatures other than 25 degrees Celcius?

A

By comparing the concentrations of hydroxide to hydronium ion

31
Q

Strong acids are assumed to ….

A

dissociate completely unless otherwise stated

32
Q

Strong acids examples

A 
HCl
HBr
HI
HClO4
HClO3
HNO3
first H in H2SO4
33
Q

Strong acid dissociation

A

HCl + H2O –> Cl- + H3O+

34
Q

In pure water at 25 degrees Celsius, the concentration of OH- and H3O+ is equivalent to…

A

1.0 * 10 ^ -7 M

35
Q

Strong bases are assumed to …

A

dissociate completely unless otherwise stated

36
Q

Strong acids dissociate in water to produce …

A

H3O+ ions

37
Q

Strong bases to dissociate in water to produce …

A

OH- ions

38
Q

The net ionic equation for the mixing a strong acid and strong base is ….

A

OH- + H+ –> H2O

39
Q

The neutralization reaction for mixing a strong acid and strong base is …

A

Strong acid + Strong Bases —> Water + Salt

40
Q

Group 1 hydroxides include …

A

Oh

41
Q

Group 2 hydroxides include …

A

Oh

42
Q

When acids dissociate, only one …

A

“H’ is dissociate at a time.

43
Q

[H3O+] is also known as …

A

H+

44
Q

pH < pKa

A

acid has a higher concentration in the original solution

45
Q

pH > pKa

A

conjugate acid has a higher concentration in the original solution

46
Q

acid-base indicator

A

any substances that exhibit different properties in protonated/ deprotonated states
RESPOND to pH

47
Q

Equivalence point

A

of moles of titrant added is EXACTLY sufficient to react completely with # of moles of titrated species

48
Q

End point

A

point in titration at which indicator undergoes its color change

49
Q

At the equivalence point pKa can be determined by…

A

taking the -log of Ka

50
Q

At the equivalence point pKb can be determined by…

A

taking the -log of Kb

51
Q

A titration graph of a weak acid titrated with a strong base looks like ….

A

forward “S”

52
Q

A titration graph of a weak base titrated with a strong acid looks like…

A

backward “S”

53
Q

Molecular structure of stronger acids

A

weak H-X bond where X is another element

54
Q

Molecular structure of weaker acids

A

strong H-X bond where X is another element

55
Q

Oxoacids/ Oxyacids

A

Contain an atom bonded to one or more oxygen atoms

56
Q

inductive effect

A

Attraction of electrons in adjacent bonds by more electronegative atoms

57
Q

Strong acids experience an inductive effect due to …

A

highly ELECTRONEGATIVE oxygen atoms

58
Q

Polarity in strong acids draw electrons ….

A

AWAY from H- atom causing an EASIER IONIZATION

59
Q

Weak acids do not experience a

A

STRONG induced dipole force

60
Q

Polarity in weak acids are ….

A

less than in strong acids -> stronger bond between H+ and oxygen atom -> LESS IONIZABLE

61
Q

If conjugate bases are less stable then…

A

a stronger base will result

62
Q

Stronger acids results in …

A

Weaker bases

ap chemistry (9 decks)

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