1.1/2.5 water and the fitness of the environment Flashcards

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1
Q

hydrogen bond definition

A

O- bonds with H+ on a different molecule of H2O

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2
Q

how many bonds can H2O form?

A

4

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3
Q

cohesion definition

A

polar H-bonding between like molecules

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4
Q

surface tension definition

A

measure of difficulty to break or stretch surface of liquid (H-bonding)

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5
Q

adhesion definition

A

H-bonding between unlike molecules

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6
Q

how does adhesion of water to vessel walls work?

A

Adhesion of H2O to vessel walls counters downward pull of gravity

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7
Q

transpiration definiton

A

movement of H2O up plants

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8
Q

how does water move up plants?

A

H2O clings to each other by cohesion; cling to xylem tubes by adhesion

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9
Q

heat definition

A

total amount of KE in system

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10
Q

temperature definition

A

measure intensity of heat due to average KE of molecules

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11
Q

water’s high specific heat:

A

Change temp less when absorbs/loses heat
Large bodies of water absorb and store more heat/energy → warmer coastal areas
Create stable marine/land environment
Humans ~65% H2O → stable temp, resist temp. change
H-bonding

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12
Q

evaporative cooling

A

Water has high heat of vaporization
Molecules with greatest KE leave as gas
Stable temp in lakes & ponds
Cool plants
Human sweat
liquid –> gas

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13
Q

insulation by ice

A

less dense, floating ice insulates liquid H2O below

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14
Q

solution

A

liquid, homogeneous mixture of 2+ substances

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15
Q

solvent

A

dissolving agent (liquid)

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16
Q

what’s the best versatile solvent?

A

water

17
Q

solute

A

dissolved substance

18
Q

hydrophilic solvents

A

affinity for H2O
polar, ions
cellulose, sugar, salt
blood

19
Q

hydrophobic solvents

A

repel H2O
nonpolar
oils, lipids
cell membrane

20
Q

hydronium ion production

A

H+ + H2O –> H3O+

21
Q

hydroxide ion production

A

H2O - H+ –> OH-

22
Q

acid definition

A

increases [H+]

23
Q

base definition

A

reduces [H-]

24
Q

what pH are most biological fluids?

A

6-8

25
Q

pH =

A

-log [H+]

26
Q

calculating pH formula

A

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

27
Q

buffers definition

A

minimize changes in concentration of H+ and OH- in a solution (weak acids and bases)

28
Q

pH of blood

A

7.4 (about) - maintained by buffers

29
Q

deadly blood pH?

A

less than 7, over 7.8

30
Q

what are important buffers in blood plasma?

A

carbonic acid – bicarbonate system

31
Q

carbonic acid decomposition

A

H2CO3 (carbonic acid) –> HCO3- (bicarbonate) + H+

32
Q

CO2 + seawater

A

carbonic acid