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Chemistry SL > Chapter 8, 9, 10, 11 > Flashcards

Chapter 8, 9, 10, 11 Flashcards

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1
Q

what color does litmus turn for acidic & alkaline solutions?

A

acidic = red
alkaline = blue

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2
Q

what color does phenolphthalein turn for acidic & alkaline solutions?

A

acidic = colourless
alkaline = pink

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3
Q

what color does methyl orange turn for acidic & alkaline solutions?

A

acidic = red
alkaline = yellow

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4
Q

strong vs concentrated

A

strong = completely dissociated into ions
concentrated = high number of moles of solute per litre of solution

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5
Q

meaning of corrosive

A

chemically reactive

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6
Q

weak acids

A

ethanoic acid (CH3COOH)
carbonic acid (H2CO3)
phosphoric acid (H3PO4)
sulfurOUS acid (H2SO3)
nitrOUS acid (HNO2)

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7
Q

strong acids

A

HCl
nitrIC acid (HNO3)
sulfurIC acid (H2SO4)
HBr
HI
perchloric acid (HClO4)
chloric acid (HClO3)

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8
Q

What is the H+ concentration of 0.0100 M H2SO4?

A

0.0100 x 2 = 0.0200 M

remember to use this ^ value for pH calculations

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9
Q

examples of neutralisation reactions?

A

acid & metal hydroxide
acid & metal oxide
acid & base
acid & metal carbonate
acid & metal hydrogen carbonate

NOTTTTT ACID & METAL NO

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9
Q

examples of neutralisation reactions?

A

acid & metal hydroxide
acid & metal oxide
acid & base
acid & metal carbonate
acid & metal hydrogen carbonate

NOTTTTT ACID & METAL NO

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10
Q

outline one application of oxidising agents

A

can be used as disinfectants

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11
Q

why is the use of chlorine as a disinfectant of concern?

A

due to its ability to oxidise other species forming harmful by-products (e.g. trichloromethane)

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12
Q

where does oxidation occur for BOTH voltaic & electrolytic cells?

A

at the ANODE

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13
Q

where does reduction occur for BOTH voltaic & electrolytic cells?

A

at the CATHODE

RUKAYA ATE COOKED AARDVARKS

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14
Q

distinguish b/w voltaic & electrolytic cells

A

VOLTAIC (galvanic) = SPONTANEOUS, convert chemical energy –> electrical energy
CPRANO

ELECTROLYTIC = NON-SPONTANEOUS, convert electrical energy –> chemical energy
PANCake

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15
Q

How is a redox reaction used to produce electricity in a voltaic cell?

A
  • e.g. zinc half cell connected to copper half cell
  • zinc is higher in activity series than copper so electrons will flow from zinc half cell to copper half cell
  • zinc electrode eventually gets smaller (as solid zinc goes into solution as Zn2+)
  • Cu electrode gradually gets larger as it becomes coated w/ copper (Cu2+ ions in sol pick up the electrons to form solid Cu)
  • COLOUR OF SOLUTION IN CU HALF CELL BECOMES PALER AS COPPER IONS BECOME COPPER ATOMS
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16
Q

what does voltage produced depend on (voltaic cell)?

A
  • depends on relative difference b/w the 2 metals in the activity series
  • greater distance on activity series = higher voltage
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17
Q

function of salt bridge

A

completes the circuit & keeps the half cells electrically neutral
negative ions go into Zn half cell
positive ions go into Cu half cell

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18
Q

consequences of NO salt bridge

A
  • buildup of Zn2+ ions in left beaker –> solution becomes positive overall, no more oxidation of Zn to Zn2+
  • decrease in Cu2+ concentration in right beaker –> solution would have negative charge & further reduction of Cu2+ ions would be opposed
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19
Q

which metal will be the negative electrode in the voltaic cell (anode)?

A

the more reactive metal will have the greater tendency to be oxidised & will be the anode

20
Q

what does the single vertical line represent?

A

phase boundary (b/w solid & aq sol)

21
Q

what does the double line represent?

A

the salt bridge

22
Q

define electrolysis

A

the breaking down of a substance (in molten state or solution) by the passage of electricity through it

23
Q

why electrodes usually made of graphite?

A

it is a fairly inert non-metal which conducts electricity

24
Q

define electrolyte

A

a solution or molten compound that will conduct electricity, with decomposition at the electrodes as it does so

contains IONS that are free to move towards the electrodes

25
Q

How do electrolytic cells carry an electric current?

A
  • battery provides source of electrical energy
  • pushes electrons onto the cathode, making it negatively charged
  • electrons are drawn OUT of the anode, making it positively charged
  • at the anode, oxidation occurs, releasing electrons that are then attracted to the positively charged anode
  • at the cathode, reduction occurs, which uses up the electrons that are building up on the cathode
26
Q

one application of electrolysis

A

used to obtain reactive metals, such as sodium, from their common ores

27
Q

Define BOD

A

the amount of oxygen used by aerobic microorganisms in water to decompose the organic matter in water over a fixed period of time (~5 days) at a fixed temperature (~20C)

28
Q

BOD levels

A

1-3 very good
3-5 moderately clean
6-9 poor (some microorganisms present)
100+ very polluted

29
Q

What is the oxidation state of sulfur in (S4O6)2- ?

A

+2.5

30
Q

What are random uncertainties caused by?

A

caused by limitations of the measuring apparatus & other uncontrollable variables that are inevitable in any experiment

30
Q

What are random uncertainties caused by?

A

caused by limitations of the measuring apparatus & other uncontrollable variables that are inevitable in any experiment

31
Q

how can effects of random uncertainties be limited?

A
  • conducting repeat trials / measurements
  • careful design of experiment
  • can never be completely eliminated
32
Q

uncertainties are usually quoted to how many sig figs? for analog instruments

A

usually 1 sig figs only

remember: half the smallest division to which you take a reading

33
Q

e.g. of human limitation

A

reaction time

34
Q

define precision

A

a measure of how close a series of measurements are to one another

35
Q

define accuracy

A

how close a measurement is to the actual value of a particular quantity

36
Q

what causes systematic errors?

A

occur as a result of a flaw in the experimental design or apparatus

cannot be reduced by conducting repeat trials

37
Q

equation for percentage error

A

percentage error = (experimental value - theoretical value) / theoretical value
x 100

If the experimental value is less than the theoretical value, the percentage error will be negative & vice versa

38
Q

equation for percentage uncertainty (%)

A

(absolute uncertainty / measurement) x 100%

39
Q

how to calculate uncertainty of the mean?

A

take the uncertainty of the mean to be 2/3 of the deviation from the mean

40
Q

when quantities w/ uncertainties are added or subtracted. . .

A

the ABSOLUTE uncertainties are ADDED

41
Q

when quantities w/ uncertainties are multiplied or divided. . .

A

the PERCENTAGE uncertainties should be ADDED

42
Q

if 12.12 +/- 0.01 is multiplies by 3, what is the answer?

A

36.36 +/- 0.03

for division, u divide the uncertainty by 3 as well

43
Q

how to work out gradient of curve at specific point

A

draw a tangent to the curve at the desired point
work out the gradient of the tangent as usual

44
Q

IHD is. . .

A

the number of double bond equivalents

45
Q

formula for IHD

A

2x+2-y / 2

46
Q

what is the IHD of benzene?

A

4, because it has 1 ring and the equivalent of 3 double bonds

47
Q

rules for IHD

A
  1. ignore O
  2. count a halogen as a hydrogen
  3. if it has nitrogen atoms, subtract 1 hydrogen atom for every nitrogen atom, & then calculate as normal

Chemistry SL (5 decks)

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