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C4 Flashcards

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1
Q

Reaction between acid and base

A

acid + base → salt + water

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2
Q

Reaction between acid and metal

A

acid + metal → salt + hydrogen gas

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3
Q

Reaction between acid and metal carbonate

A

acid + metal carbonate → salt + water + carbon dioxide

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4
Q

Excess method of salt preparation

A

Involves the addition of an excess of an insoluble base (metal, metal oxide or metal carbonate).

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5
Q

Insoluble base + acid reaction

A

insoluble base + acid → soluble salt

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6
Q

Steps for excess method of salt preparation

A
  1. Warm the acid
  2. Add the insoluble base to excess to ensure all the acid has reacted
  3. Filter off the excess insoluble base
  4. Heat solution to evaporate half of the water
  5. Leave to cool and crystallise
  6. Dry the crystals
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7
Q

Why is the insoluble base added to excess in the excess method of salt preparation?

A

To make sure all of the acid reacts.

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8
Q

Titration method for salt preparation

A

Involves the addition of an acid to an alkali using a burette.

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9
Q

Titration reaction

A

soluble base (alkali) + acid → soluble salt + water

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10
Q

Steps for titration method of salt preparation

A
  1. Add acid in a conical flask using a volumetric pipette
  2. Fill a burette with alkali
  3. Add an indicator to the conical flask
  4. Add the alkali into the acid, slowly near the end point to find the exact volume required for neutralisation
  5. Repeat without the indicator
  6. Heat the solution to evaporate half of the water
  7. Leave to cool and crystallise
  8. Dry the crystals
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11
Q

Precipitation method for salt preparation (for insoluble salts)

A

Mix together solutions of two soluble salts to provide the ions needed.

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12
Q

Precipitation reaction

A

soluble salt + soluble salt → insoluble salt (residue) + soluble salt (filtrate)

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13
Q

Test for oxygen gas

A

Accelerates combustion reactions and relights a glowing splint.

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14
Q

Test for hydrogen gas

A

Reacts with oxygen in the air when exposed to a flame and combusts (burns) with a squeaky pop.

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15
Q

Test for carbon dioxide gas

A

Reacts with calcium hydroxide (limewater) to produce calcium carbonate, turning clear and colourless limewater milky/cloudy.

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16
Q

Test for ammonia gas

A

Reacts with litmus, turning damp red litmus paper blue.

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17
Q

Test for chlorine gas

A

Reacts with litmus, turning damp blue litmus paper red and then white/bleached.

18
Q

Ammonia gas characteristics

A

No colour, pungent (strong & nasty) smell like rotten nappies.

19
Q

Chlorine gas characteristics

A

Greenish-yellow gas with a pungent choking smell, like swimming pools.

20
Q

Flame test for lithium (Li+)

21
Q

Flame test for potassium (K+)

22
Q

Flame test for sodium (Na+)

23
Q

Flame test for copper (Cu2+)

A

Blue-green.

24
Q

Precipitation reactions to test for cations

A

When you react some cations with hydroxide or ammonia solution, a coloured precipitate can form.

25
Q

Ammonium result with aqueous sodium hydroxide

A

Ammonia gas produced on warming.

26
Q

Ammonium result with aqueous ammonium hydroxide

A

No reaction.

27
Q

Copper (II) result with aqueous sodium hydroxide

A

Light blue ppt, insoluble in excess.

28
Q

Copper (II) result with aqueous ammonium hydroxide

A

Light blue ppt, soluble in excess giving a dark blue solution.

29
Q

Iron (II) result with aqueous sodium hydroxide

A

Green ppt, insoluble in excess.

30
Q

Iron (II) result with aqueous ammonium hydroxide

A

Green ppt, insoluble in excess.

31
Q

Iron (III) result with aqueous sodium hydroxide

A

Red-brown ppt, insoluble in excess.

32
Q

Iron (III) result with aqueous ammonium hydroxide

A

Red-brown ppt, insoluble in excess.

33
Q

Zinc (II) result with aqueous sodium hydroxide

A

White ppt, soluble in excess giving a colourless solution.

34
Q

Zinc (II) result with aqueous ammonium hydroxide

A

White ppt, soluble in excess giving a colourless solution.

35
Q

Chloride (Cl-) anion test and result

A

Acidify with dilute nitric acid, then add aqueous silver nitrate. White ppt.

36
Q

Bromide (Br-) anion test and result

A

Acidify with dilute nitric acid, then add aqueous silver nitrate. Cream ppt.

37
Q

Iodide (I-) anion test and result

A

Acidify with dilute nitric acid, then add aqueous silver nitrate. Yellow ppt.

38
Q

Carbonate (CO3(2-)) anion test and result

A

Add dilute acid. Effervescence, carbon dioxide produced.

39
Q

Sulfate (SO4(2-)) anion test and result

A

Acidify, then add aqueous barium nitrate. White ppt.

40
Q

Tests for water

A

Anhydrous Copper Sulfate changes from white to blue. Cobalt (II) chloride changes from blue to a light pink/purple.

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