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physical chem > acids and bases > Flashcards

acids and bases Flashcards

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1
Q

bases soluble in water

A

are alkalis

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2
Q

zinc hydroxide

A

Zn(OH)2

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3
Q

acid definition

A

any substance that adds H+ ions to water
-proton donor

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4
Q

hydronium ions

A

hydrogen atoms attach to h2o molecule to form H30

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5
Q

base definition

A

proton acceptor

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6
Q

weak acids

A

only a few molecules dissaaociste into ions

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7
Q

strong acids

A

molecules completely dissociate into ions

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8
Q

strong base

A

fully dissociate

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9
Q

weak bases

A

react with water to form equilibrium with h2o

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10
Q

conjugate acid

A

base plus h+

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11
Q

conjugate base

A

acid reacting with base and donating proton

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12
Q

equation for concentration

A

moles of ion concentration/ volume of solution

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13
Q

pH =

A

-log10(H+)

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14
Q

increasing conc if acid

A

decreases pH value

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15
Q

pH of strong acid

A

-log10(H+)

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16
Q

conc of strong acid

A

(H+) = 10-pH

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17
Q

moles with conc and volume

A

conc times volume

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18
Q

acid solution + aqueous base when calculating new pH

A

find change in volume
-find change in (H+)

19
Q

Kc =

A

products over reactants

20
Q

Kw =

A

H+ times OH-
units mol 2 dm-6

21
Q

equation for dissociation of water

A

H2O – H+ + OH-

22
Q

Kw at room temp

A

1 times 10-14

23
Q

temperature effect on kW

A

decreases if H and OH decrease and if conc of H and OH increase it increases

24
Q

why does Kw change when temp increases

A

because equilibrium shifts to right so conc of H and OH produced increases so larger number brings value of Kw up and goes down if conc decreases
-position shifts to right because ionisation of water endothermic

25
Q

how to find conc of H+ ions in equation

A

-H and OH equals H squared
-to find H conc you have to square root KW value

26
Q

why is pure water always neutral

A

hydrogen ions always equal to amount of hydroxide ions

27
Q

how to work out conc of OH or H when kW given and one other concentration given

A

Kw divided by other concentration

28
Q

what doesnt affect Kw value of pure water

A

conc of H and OH ions
-addition of base to water
-addition of acid to water
pH

29
Q

finding pH of strong acid

A

-log10 H+

30
Q

finding pH of strong base

A

-first find the concentration of OH ions using dissociation equation
-find conc of H+ of ions
-use Kw to find it - rearrange equation of Kw
-

31
Q

dissociation of NaOH

A

NaOH = Na+ + OH-

32
Q

calculating conc of strong base

A

use pH to find conc of H ions
-10-ph
-use Kw to find conc of OH ions
-OH = Kw/ H+

33
Q

pH and group 2 hydroxides

A

times by 2 because 1-2 ratio

34
Q

solubility going down group 2

A

increases

35
Q

factors that affect pH of solution

A

amount of dissociation
-solubility
-concentration of H+ ions
-temperature

36
Q

calculating what mass of molecule dissolved into water

A

-use pH to find conc of solution
–logH+
-then OH= Kw/ H+
-rearrange to get moles= conc times volume
-mass= moles times molar mass

37
Q

calculating final pH of two solutions

A

-find moles of both compounds
-which one is in excess- calculate limiting compound leftover after reaction
-find conc of limiting in final solution
-use Kw to find conc of opposite ion in final solution
-use conc to find pH

38
Q

whats a buffer

A

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

39
Q

what must buffer solutions have

A

high concentrations of undissociated acids and high concs of its conjugate base

40
Q

exam question how does a buffer resist changes in pH upon addition of a small amount of acid

A

write down reversible reaction for specific buffer
state that adding acid increases H+
state that equilibrium shifts to the left to lower the conc of H+
state that overall H+ remain almost constant

41
Q

exam question how does a buffer resist changes in pH upon addition of small amount of base

A

write down reversible reacrtion for specific buffer
state that reacrion takes place between OH- and H+ which lowers the conc of H+ ions in buffer solution
state that equilibrium shifts to right to replenish lost H+
state that overall H+ remains almost constant

42
Q

use of buffers in real life

A

brewing of beer
blood- hydrogencarbonate
swimming pools

43
Q

alkaline buffers

A

weak base and conjugate acid
pH below 7

44
Q
A

physical chem (10 decks)

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