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MCAT General Chemistry > Chapter 10: Acids and Bases > Flashcards

Chapter 10: Acids and Bases Flashcards

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1
Q

An Arrhenius acid dissociates to form ____.

A

H+ ions

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2
Q

An Arrhenius base dissociates to form ____.

A

OH-

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3
Q

A Bronsted acid ____________ H+

A

donates

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4
Q

A Bronsted base ____________ H+

A

accepts

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5
Q

Bronsted-Lowry acids and bases always occur in pairs because the definitions requires what?

A

The transfer of a proton from the acid to the base, aka conjugate acid-base pairs

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6
Q

A conjugate acid is ____.

A

a base with a hydrogen ion added to it

in the reverse reaction, it is the H+ donor, thus it is an acid

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7
Q

A conjugate base is ____.

A

an acid with a hydrogen ion removed from it

in the reverse reaction, it accepts H+, thus it is a base.

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8
Q

An ____________ species is one that reacts like an acid in a basic environment and like a base in an acidic environment.

A

amphoteric

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9
Q

In the Bronsted-Lowry sense, an amphoteric species can either gain or lose a proton, making it ____________ as well

A

amphiprotic

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10
Q

The partially dissociated conjugate base of a ________________ acid is usually amphoteric, e.g. HSO4-. The ____________ of certain metals, e.g. Al, Cr, Pb, Zn, are also amphoteric.

A

polyvalent; hydroxides

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11
Q

Complex amphoteric molecules include amino acids that have a ____________ intermediate with both cationic and anionic character.

A

zwitterion

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12
Q

Acids formed from anions with names that end in -ide have the prefix ________ and the ending ____.

A

hydro-
-ic

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13
Q

Acids formed from oxyanions are called oxyacids.
If the anion ends in -ite (less oxygen), then the acid will end in ________. If the anion ends in -ate (more oxygen), then the acid will end with ____ acid.

A

-ous acid
-ic acid

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14
Q

What is the only thing that can affect Kw?

A

temperature! just like any other equilibrium constant

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15
Q

At temperatures above 298 K, Kw will increase. Why?

A

The autoionization reaction is endothermic

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16
Q

Strong acids and bases do what in aqueous solutions?

A

Completely dissociate

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17
Q

What do weak acids and bases do in aqueous solutions?

A

They partially dissociate

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18
Q

The smaller the Kb or Ka, the (stronger/weaker) a base or acid is.

A

weaker

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19
Q

Electronegative elements positioned near an acidic proton increase acid strength how?

A

they pull electron density out of the bond holding the acidic proton - this weakens proton bonding and facilitates dissociation

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20
Q

Acids and bases may react with each other to form a salt and often (not always) water. This is a ____________ reaction.

A

neutralization

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21
Q

In acid-base titrations, the equivalence point is reached when what?

A

the # of acid equivalents present equals the number of base equivalents, or vice versa

22
Q

THe point at which the indicator changes to its final color is not the equivalence point, but rather the ____________

A

endpoint

23
Q

Main differences between strong acid vs weak acid titration with strong base?

A
  1. initial pH is greater
  2. strong acid has steeper/sudden rise in pH
  3. equivalence point is greater than 7
24
Q

Why do weak acid strong base titrations have pH > 7?

A

produces a weak conjugate base and even weaker conjugate acid - this means there are more OH- than H3O+

25
Q

A ____________ ____________ consists of a mixture of a weak acid and its salt (which is composed of its conjugate base and a cation) OR a mixture of a weak base and its salt.

A

buffer solution

26
Q

What are two major examples of buffers?

A

CH3COOH and CH3COO-Na+
NH3 and NH4+Cl-

27
Q

What is an important property of buffers?

A

Can resist changes in pH when small amounts of acid or base are added

28
Q

One of the most important buffers in the human body is the ________________ buffer system.

A

bicarbonate

29
Q

In metabolic acidosis, what occurs?

A

Increased breathing to deplete CO2 and shift the system to the left to reduce H+

30
Q

What would happen if concentrations of both the acid and its conjugate base were doubled in a buffer solution?

A

THe buffering capacity, or ability to which the system can resist changes in pH, would increase

31
Q

Oxidation is ________

A

loss of e-

32
Q

Reduction is ________

A

gain of e-

33
Q

An oxidizing agent causes what?

A

Causes an atom to be oxidized, and is itself reduced

34
Q

A reducing agent causes what?

A

Causes an atom to be reduced, and is itself oxidized

35
Q

Almost all oxidizing agents contain what?

A

oxygen or another strongly electronegative element

36
Q

What are some common oxidizing/reducing agents?

A
37
Q

________________ ____________ are assigned to atoms to keep track of redistribution of electrons during chemical reactions

A

Oxidation numbers

38
Q

What is the oxidation number of a free element?

A

Zero

39
Q

The oxidation number of a monatomic ion is equal to what?

A

The charge of the ion

40
Q

The oxidation number of Group VIIA is -1, except for when?

A

When combined with an element of higher electronegative.

Example: Cl- is -1 in HCl, but it is +1 in HOCl

41
Q

Hydrogen is usually ____. However, it is ____ in compounds with less electronegative elements from Groups ____ and ____.

Hydrogen is ____ in HCl, but ____ in NaH.

A

+1; -1; Groups IA and IIA
+1, -1

42
Q

In most compounds, the oxidation number of oxygen is ____. Except in peroxides (O22-), where oxygen is ____, and compounds with more electronegative elements like OF2, where oxygen is ____.

A

-2; -1, +2

43
Q

The sum of oxdiation numbers in a neutral compound should be ____

A

zero

44
Q

The sum of oxidation numbers of the atoms present in a polyatomic ion is equal to ____

A

the charge of the ion

45
Q

Oxidation number assumes ________ ________ of electrons in bonds, “awarding” the electrons to the more electronegative element.

A

unequal division

46
Q

Formal charge assumes ________ ________ of electrons in bonds, awarding one electron to each atom in the bond.

A

equal division

47
Q

When assigning oxidation numbers, start with what?

A

The known atoms

48
Q

What does assigning oxidation numbers accomplish?

A

Allows us to determine how many moles of each species are required for conservation of charge and mass, which is necessary to balance the equation

49
Q

How does the half-reaction method work?

A

Separate the redox reaction into two half-reactions, the oxidation part and the reduction part, then they are balanced separately

50
Q

________________ is a specific type of redox reaction in which an element undergoes both oxidation and reduction in producing its products.

A

disproportionation

51
Q

What is an example of disproportionation?

A

catalysis of peroxides by catalase

MCAT General Chemistry (12 decks)

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