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CHEM 301 > LECTURES 5-8 + TBL 2 > Flashcards

LECTURES 5-8 + TBL 2 Flashcards

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1
Q

In aqueous systems, CO2 exists as a combination of _____, _____, _____

A

CO2, HCO3, H2CO3, CO3

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2
Q

The sum of all species that form when CO2 reacts with water (CO2 + HCO3 + CO3)

A

dissolved inorganic C (DIC) / total CO2

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3
Q

our atmospheric CO2 has risen from ____ppm to _____pm from the pre-industrial times up until now

A

278, 420

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4
Q

about _____% of known CO2 emissions are no longer in the atmosphere, and rather in the ocean

A

40

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5
Q

the liquid that dissolves the solute

A

solvent

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6
Q

the solid dissolved in the liquid

A

solute

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7
Q

the quantity of solute relative to that of solvent/solution

A

concentration

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8
Q

produce H+ ions (or H3O) and have a pH < 7

A

acids

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9
Q

produce OH- ions and have a pH >7

A

bases

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10
Q

a stress placed on a system in equilibrium will shift the equilibrium to relieve the stress

A

Le Chatelier’s Principle

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11
Q

takes into account the ionic strengths and ion size and charge; are more accurate than concentrations in equilibrium, but are approximately equal at low ionic strengths (freshwater)

A

activity coefficient

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12
Q

[H+][OH-] = 10^-14

A

water dissociation constant

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13
Q

the henderson hasselbach equation explains that when adding ____, it comes with the weak base to form the acid, which shifts the ratio but only has a small effect on ____

A

H+, pH

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14
Q

buffers work best when the pH is near the _____ of the acid, where _____ = _______

A

pka, [HA], [A]

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15
Q

total hydroxide ion concentration; manifested by a high pH

A

basicity

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16
Q

the capacity of water to accept H+; determined by titration with H+ to neutral endpoint; includes the concentration of all conjugate bases of weak acids

A

alkalinity

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17
Q

when the pH of water equals the pka1 or _____, the concentration of _____ and _____ are equal to each other

A

6.35, CO2, HCO3

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18
Q

when the pH of water equal the pka2 or ______, the concentration of _____ and _____ are equal to each other

A

10, HCO3, CO3

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19
Q

at maximum HCO3 concentration, there is very little _____ and_____

A

CO2, CO3

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20
Q

at pH ____, it is almost all CO2, at pH ____, it is almost all CO3

A

<4, >12

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21
Q

the pH of freshwater is around __, which is buffered by CO2 and HCO3, with mostly ______ existing in the water

A

7, HCO3

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22
Q

due to the high ____ content and thus _____ strength, the pka2 in the ocean is ____. seawater is at a pH of _____ and well buffered. Adding anthropogenic CO2 will cause ____ to decrease,, pH to ____ and make it difficult for ____ to grow and harder to ___ future changes with additional CO2

A

salt, ionic, 9.4, 8, CO3, decrease, corals, buffer

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23
Q

includes only those species present when CO2 is added to pure water: CO3, HCO3, OH-, H+ (can ignore [OH] or [H] in pH < 7 or pH > 7 respectively)

A

carbonate alkalinity

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24
Q

the combined total when other bases contribute to the alkalinity

A

total alkalinity

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25
Q

____ water can absorb more CO2 than neutral water; a low [H+] means that a shift in reaction to the right results in _____ CO2 dissolved, increased, _____ and _____ alkalinity

A

basic, more, DIC, increased

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26
Q

water gains alkalinity primarily due to dissolution of _____, which increases ______ forms of DIC, and increases the_____

A

CaCO3, basic, pH

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27
Q

measure of “mineral” content of water (dissolved solids/ions)

A

water hardness

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28
Q

____ is generally the highest concentration of all cations in freshwater systems, although ____ can also contribute. Water with more ____ can dissolve more Ca minerals, which means it is dependent on T, ____, ____, _____, respiration and ____

A

Ca2+, Mg2+, CO2. P, S, pH, PS

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29
Q

Vancouver has the _____ water, with <_____mg/l, because the coast mountains mostly contain ______

A

softest, 3, granite

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30
Q

occurs when Ca2+ complexes with soap to form a neutral species, which makes soap insoluble in water, instead of soluble due to the exposed ionic end of the O-

A

scum

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31
Q

Deposits of CaCO3 that form when hard water is boiled due to increase of temperature which forms the precipitate, and due to the fact that less CO2 can be dissolved

A

scale

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32
Q

added CO2 to the oceans results in carbonic acid, which releases a _____. The _____ absorbs that proton, which means the overall ____ concentration decrease. This makes it difficult for marine organisms to use it for their ____

A

proton, CO3, carbonate, shells

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33
Q

_____ ____ caused by neighbouring coal mining industries are mostly a problem of the past because it is a _____ source, which means it can be treated there. However, below a pH of _____, Al ions are mobilized from insoluble clay minerals to a dissolved and _____ form which kills fish

A

acid rain, point, 5, bioavailable

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34
Q

_____ _____ with high sulfur content, results in emission of _____ causing acidification due to the production of ______, can be regulated. _____ also becomes _____ and results in acidification

A

dirty coal, SO2, H2SO4, NO2, HNO3

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35
Q

CO2 is a _____ acid because it becomes _____, which has a pka of 6.35, making it impossible to bring pH’s down to 5. For a low pH, you need a ____ acid and little ______

A

weak, H2CO3, strong, buffering

36
Q

Most NO2 comes from reactions of N2 and O2 in the atmosphere due to

A

internal combustion engines

37
Q

As ____ is a limiting factor of primary productivity in some areas of the ocean, adding some of it could stimulate enough PP to consume ____ of the anthropogenic flux of CO2

A

Fe, 1/3-1/2

38
Q

in the surface, CO2 is taken up by ____ which creates ______ (phytoplankton biomass). When it dies, it _____, then _______ through respiration and decomposition, which releases CO2 as _____. A small fraction of this settles to the _____. The slow mixing between the deep and surface results in most of the released CO2 to stay in the ______. Upwelling and ______ circulation eventually bring CO2 back up to the surface but it takes a long time

A

photosynthesis, particulate organic matter, sinks, oxidizes, DIC, sediments, deep, thermohaline

39
Q

How _____ CO2 goes down to the oceans affects how long before it re-enters the atmospheres, as deeper oceans take 1000s-millions of years for re-release

A

far

40
Q

With added Fe, phytoplankton _____ were created, but the damages to the ______ were uncertain. Furthermore, the Fe oxidizes in water and turns ____, which brings uncertainty as to whether it was fully absorbed

A

blooms, ecosystem, red

41
Q

The artificial modification of the Earth’s climate systems through 2 primary ideologies: carbon dioxide removal, and solar radiation management (does nothing for ocean acidification)

A

geoengineering

42
Q

compressing CO2 to a liquid form which coverts to clathrate hydrates over time and flows down into CO2 lakes

A

ocean CO2 injection

43
Q

other methods of CO2 involves combining it with _____ to get a less harmful ______, dispersing it by _____, or getting it to be absorbed by a ____ first then removing it, as well as pumping it into rock under the sea floor off ______

A

carbonate, bicarbonate, ships, mineral, island

44
Q

there is uncertainty that accompanies specific predictions of _______ impacts of increased levels of CO2, even though there is consensus in the scientific community on the calamity caused by ____ _____

A

environmental, fossil fuels

45
Q

the 4 major ions in river water

A

Ca2+, Mg2+, Na+, K+

46
Q

potentially toxic natural trace metals that are controlled primarily by the solubility of their hydroxides and carbonate salts

A

minor ions

47
Q

____ pH water had higher concentration of trace metals, as it makes _____ and ____ more soluble

A

low, hydroxides, carbonates

48
Q

the metal ions of most interest for trace metals

A

Cr3+, Mn(2+/4+), Fe(2+/3+)

49
Q

most properties of metals dissolved in water depend on the _____ of the metal; ____ ____ ____ and ____ all change with speciation. thus we cannot just determine how much total metal is present

A

chemical form/metal species, solubility, mobility, toxicity, bioavailability

50
Q

a central metal cation (electron acceptor or lewis acid), surrounded by anions of molecules containing free pairs of electrons (electron donor, or Lewis base)

A

coordination complex

51
Q

anions or molecules providing the free pair of electrons

A

ligands

52
Q

the metal-ligand bond

A

coordinate covalent bond

53
Q

In order for a complex to be formed from one or more ligands and a central atom, each ligand must possess at least one _______ and the central atom must be able to accept it from each ligand

A

unshared electron pair

54
Q

a ligand with a single pair of available electrons

A

monodentate ligand

55
Q

ligand molecules containing more than one ligand atom

A

multidentate ligands

56
Q

a metal complex in which the ligand molecule has multiple donor sites that are sufficiently spaced so they can bind to the same metal ion, and forms 5 or 6 membered rings when bound to a metal so that there are no unstable bond angles

A

Chelate

57
Q

the number of ligand atoms per central atom

A

coordination number

58
Q

the stability of chelates increases with each additional ______ atom, which are typically in organic molecules, ____, ___, and ____

A

donor, O, N, S

59
Q

a chelating agent with 6 donor atoms (4 Os and 2 Ns) that is a common food additive, pollutant, and therapy method

A

EDTA

60
Q

complexation generally _____ bioavailability, and ______ their concentration in water when in contact with solid forms (due to increased solubility)

A

decreases, increases

61
Q

Chelating ligands _____ metals due to increasing its solubility, and thus if transported to a different environment, can ____ the metal

A

transport, release

62
Q

While some chelating ligands may be helpful to make a ____ element less bioavailable, it can also be deprived of essential ______

A

toxic, nutrients

63
Q

halogens must be ______ halides in order to function as a donor atom

A

free

64
Q

metals that have d^0 configuration and low polarization such as Na+, K+, Mg2+, Ca2+, Sc3+, Ti4+ and Al3+

A

a type metal ions

65
Q

metals that have d^1 - d^9 configuration transition metals, with a character in between A and B-type metals, such as Cr3+, Mn2+, Co2+, Fe2+, Ni2+, and Cu2+

A

intermediate metals

66
Q

metals that have a d^10 of nd^10(n+1)s^2 configuration and high polarizability such as Ag+, Au+, Hg2+, etc

A

b type metal ions

67
Q

examples of a type ligands

A

O in SO4, CO3, OH and N in organics, and F

68
Q

examples of b type ligands

A

Cl, S in HS and S in organic molecules

69
Q

the ease with which the electron density of a species can be deformed by an external influence

A

polarizability

70
Q

ligand preference order for a type metals (opposite for b type metals)

A

F > O > N > Cl > Br > I > S

71
Q

the constant for the forward rate of a complexation over the reverse rate of a complexation

A

formation constant

72
Q

a ligand that is similar to the metal type will _____ the Kf

A

increase

73
Q

chelates have a high_____ due to a slow ____; this is because multiple ____ need to break for the complex to come apart, which means both bonds need to be at the _____ point

A

Kf, Kr, bonds, weakest

74
Q

_______ ligands are easy to pull apart, as they only contain _____ site to complex with the metal, and are not connected to each other. Thus you only have to consider the _____

A

monodentate, one, Kf

75
Q

the more the d orbital is close to being filled. the more the. ion likes to complex and is in need of the extra electron density; thus, d^10, and d^5 do not complex as well as d^9

A

irving williams order

76
Q

complexation can either form _______ compounds and remove metal ions from solution, or more commonly, can form ____ compounds with insoluble metals and mobilize them (if the solid phase is in contact with the solution)

A

insoluble, soluble

77
Q

complexes are more stable if they are ______, have similar ______ and ______, have nearly complete _______, and the ligands are _______

A

higher charge, ligand, metals, d orbitals, multidentate

78
Q

Repulsion of protons from water

A

hydrolysis

79
Q

OH2 complexes

A

aquo

80
Q

OH complexes

A

hydroxo

81
Q

O complexes

A

oxo

82
Q

hydrolysis is enhanced by the _____ on metal ions, as a stronger interaction with O means H+ will leave better; lower _____ will also result in more ____ in the solution, resulting more _____ complexes

A

positive charge. pH, H+, hydrated

83
Q

increasing _____ of the metal ion increases the _____ of the O-H bond making it easier to leave; _____ also affects the type of complex formed

A

electronegativity, polarity, temperature

84
Q

species that are z=1 charge will only be _____, species that are z = 7 will only be ______, species that are between those will be combination of all three

A

aquo, oxo

85
Q

able to function as an acid or a base

A

amphoteric, metal hydroxides

CHEM 301 (7 decks)

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