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chemistry > qualitative analysis > Flashcards

qualitative analysis Flashcards

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1
Q

flame test lithium

A

red

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2
Q

flame test sodium

A

yellow

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3
Q

flame test potassium

A

lilac

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4
Q

flame test calcium

A

orange-red

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5
Q

flame test copper

A

blue-green

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6
Q

test for carbon dioxide

A

bubbling through limewater (turns cloudy)

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7
Q

why must the test for any ion be unique?

A

so you can determine which ion is present without confusion, if the test is not specific, another test would be required to determine the ion

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8
Q

carbonate ion test

A

two centimetres of the solution being tested
add a few drops of dilute hydrochloric acid

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9
Q

testing for sulphate ions

A

two centimetres of the solution being tested
add a few drops of dilute hydrochloric acid and shake
add a few drops of barium chloride

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10
Q

halide ion test

A

two centimetres of the solution being tested
add a few drops of dilute nitric acid and shake
add a few drops of silver nitrate

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11
Q

carbonate ion positive test

A

bubbling occurs

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12
Q

sulphate ion positive test

A

white precipitate forms

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13
Q

chloride ion halide test positive result

A

white precipitate forms

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14
Q

bromide ion halide test positive result

A

cream precipitate forms

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15
Q

iodide ion halide test positive result

A

yellow precipitate forms

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16
Q

cation precipitate test

A

two centimetres of the solution being tested
add a few drops of sodium hydroxide and shake
observe precipitate formed (if white complete next step)
fill the tube about halfway with sodium hydroxide

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17
Q

copper precipitate test

A

blue

18
Q

iron (II) precipitate test

A

green

19
Q

iron (III) precipitate test

A

brown

20
Q

calcium precipitate test

A

white (stays the same/remains cloudy when excess sodium hydroxide is added)

21
Q

aluminium precipitate test

A

white (turns colourless when excess sodium hydroxide is added)

22
Q

ammonium ion test

A

two centimetres of the solution being tested
add a few drops of dilute sodium hydroxide
warm the mixture
hold damp red litmus paper over the test tube

23
Q

ammonium ion positive result

A

litmus paper turns blue

24
Q

chlorine gas test

A

hold damp blue litmus paper over the mouth of the test tube which is filled with the gas being tested

25
Q

chlorine gas positive result

A

litmus paper turns red

26
Q

ammonia gas test

A

hold damp red litmus paper over the mouth of the test tube which is filled with the gas being tested

27
Q

ammonia gas positive result

A

red litmus paper turns blue

28
Q

oxygen gas test

A

test tube filled with the gas being tested
get a glowing split and hold it inside the test tube

29
Q

oxygen gas positive result

A

the glowing splint combusts and relights

30
Q

hydrogen gas test

A

test tube filled with the gas being tested
hold a lit splint over the mouth of the test tube

31
Q

hydrogen gas positive test

A

squeaky pop noise

32
Q

test for water

A

using anhydrous copper (II) sulphate which is originally white solid
add the substance being tested for water

33
Q

water positive test result

A

turns blue

34
Q

test for water purity

A

pure water should boil at 100 degrees

35
Q

water impurity positive result

A

water boils at a temperature higher or lower than 100 degrees

36
Q

what do instrumental methods of analysis improve?

A

sensitivity, accuracy and speed of tests

37
Q

which methods improve speed, accuracy and sensitivity of tests?

A

instrumental methods

38
Q

carbonate ionic equation

A

CO3^2- (aq) + 2H^+ (aq) –> CO2 (g) + H2O (l)

39
Q

sulphate ionic equation

A

Ba^2+ (aq) + SO4^2- (aq) –> BaSO4 (s)

40
Q

halide ionic equation

A

Ag+ (aq) + X- (aq) –> AgX (s)
where X = Cl^-, Br^- or I^-

41
Q

uses of a flame photometer

A

measures light intensity so you can find the concentration of ions using a calibration curve) in a dilute solution and make an emission spectra
also identify metal ions by comparing the data with reference data

chemistry (6 decks)

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