Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

y3 chem > quantitative analysis > Flashcards

quantitative analysis Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

green coloured compounds

A

copper (II) carbonate
iron (II) salts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

blue coloured compounds

A

copper (II) salts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

brown coloured compounds

A

copper metal, iron (III) compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

black coloured compounds

A

copper (II) oxide, iron (II) oxide, carbon, iodine crystals??

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

yellow coloured compounds

A

lead (II) oxide, lead (II) iodide, silver bromide, silver iodide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

cations in cation tests

A

zinc, aluminium, calcium, copper (II), iron (II), iron (III), ammonium, sodium, potassium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

solubility of zinc ions in reagents

A

white ppt (Zn(OH)2); soluble in excess
white ppt (Zn(OH)2); soluble in excess

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

solubility of aluminium ions in reagents

A

white ppt Al(OH)3; soluble in excess
white ppt Al(OH)3; insoluble in excess

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

solubility of calcium ions in reagents

A

white ppt Ca(OH)2; soluble in excess
no ppt formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

solubility of Cu2+ ions in reagents

A

blue ppt Cu(OH)2; insoluble in excess
blue ppt Cu(OH)2; soluble in excess

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

solubility of Fe2+ ions in reagents

A

green ppt Fe(OH)2; insoluble in excess
green ppt Fe(OH)2; insoluble in excess

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

solubility of Fe3+ ions in reagents

A

red brown ppt; insoluble in excess
red brown ppt; insoluble in excess

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

solubility of nh4+ ions in reagents

A

no ppt; ammonia given off upon heating
no ppt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

why dont calcium ions form a precipitate in aqueous ammonia

A

aqueous ammonia has a low concentration of OH- ions so hard for products to form, and Ca(OH)2 is partially soluble in water, meaning any product formed is likely dissolved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

why are most precipitates insoluble in excess

A

most metal hydroxides are basic and are insoluble in bases because they react with acids. exceptions are zinc and aluminium because they are amphoteric

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

anions to test for

A

carbonate, chloride, iodide, sulfate, nitrate

17
Q

how to test for carbonate ion

A

add dilute acid and bubble gas involved into limewater. a white ppt will be formed in it

18
Q

how to test for chloride ion

A

add dilute nitric acid then silver nitrate. a white ppt will be formed (AgCl)

19
Q

how to test for iodide ion

A

add dilute nitric acid then aqueous silver nitrate. a yellow ppt will be formed (AgI)

20
Q

how to test for sulfate ion

A

add dilute nitric acid then aqueous barium chloride. a white ppt will be formed (BaSO4)

21
Q

how to test for nitrate ion

A

add aqueous sodium hydroxide and aluminium. warm mixture and test with damp red litmus paper. litmus paper will turn blue because ammonia gas is produced

22
Q

processes behind nitrate ion test

A

nitrate ion is reduced to ammonium ion by aluminium, and then reacts with OH- ion in sodium hydroxide to produce ammonia gas

23
Q

why are acids added before the testing for anions

A

ascertain that carbonate ions are not present

24
Q

gases to test for

A

hydrogen, oxygen, carbon dioxide, chlorine, ammonia, sulfur dioxide??

25
Q

how to test for hydrogen

A

burning splint at mouth of test tube is extinguished with a pop sound

26
Q

how to test for oxygen gas

A

glowing splint in test tube is reignited

27
Q

how to test for carbon dioxide gas

A

bubble into water, white ppt is formed

28
Q

how to test for chlorine gas

A

place moist blue litmus paper at mouth of test tube, blue litmus paper turns red and is then bleached

gas is also yellow-green and pungent

29
Q

how to test for ammonia gas

A

place moist red litmus paper at mouth of test tube, litmus paper turns blue

30
Q

how to test for sulfur dioxide

A

place filter paper soaked with potassium manganate at mouth of test tube. potassium manganate turns colourless

31
Q

why must litmus paper be moistened for gas testing

A

allows gases to dissolve onto litmus paper to form H+ or OH- ions that cause litmus papers to change colour

y3 chem (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions