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Chemistry (N.A.) > Acids & Bases + Tests > Flashcards

Acids & Bases + Tests Flashcards

1
Q

How many protons does a hydrogen ion have

A

1 proton

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2
Q

An acid is a ____ donor?

A

Acid –> proton donor

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3
Q

What must an acid have to donate a hydrogen ion (proton)

A

An acid must have a hydrogen to donate a hydrogen ion (proton)

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4
Q

What do acids dissociate into when ____ is added?

A

They dissociate (split up) into hydrogen ions and negative ions (anions) when added to water

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5
Q

A base is a _____ _______?

A

Base –> proton acceptor

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6
Q

Bases must be able to accept a what ion?

A

Bases must accept a hydrogen ion (proton)

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7
Q

What is an alkali?

A

A soluble base

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8
Q

What do bases dissociate into when _____ is added?

A

When WATER is added, bases dissociate into hydroxide ions and positive metal ions (cations)

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9
Q

Neutralisation reactions are when…

Net ionic equation for all acid-base neutralisation reactions?

Leads to a _____ solution?

A

⭐ when acids react with alkali

⭐ H+ + OH- -> H2O

⭐ leads to a NEUTRAL solution

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10
Q

Strong Vs. Weak Acid

What does strong acid dissociate into?

Example?

A

Strong acid FULLY dissociates into water and H+ (hydrogen) ions, all hydrogen ions are donated and separate from the anions.

HCl (aq) -> H+ (aq) + Cl- (aq)

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11
Q

What does weak acid dissociate into?

Example?

What does ⇌ mean?

A

Weak acid: partially dissociates in water into H+ (hydrogen) ions, some H+ (hydrogen ions) are donated and the system forms equilibrium

CH3COOH (aq) ⇌ H+ (aq) + CH3COO- (aq)

⇌ = reversible, “can go back and forth”; a reversible reaction in which both the reactants and products are forming at the same time.

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12
Q

Does a weak or strong acid have more H+ ions?

A

Strong acids have more H+ ions in solution that weak acids.

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13
Q

Are metal oxides acidic or basic?

A

BASIC
amphoteric
dissolve in H2O

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14
Q

Are non-metal oxides acidic or basic?

A

ACIDIC
will react with an acid and be neutralised

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15
Q

What does amphoteric mean?

Examples?

A

Can react like an acid OR base

Al(OH)3
Al2O3
ZnO

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16
Q

What does amphiprotic mean?

Examples?

A

Donate AND accept hydrogen ions (H+)

H2O + H+ –> H3O+ [hydronium ion; accepting a hydrogen ion, showing water reacting like a base]

Cl- + H2O –> OH- + HCl [donates H+ to the Cl and makes HCl; acting as an acid]

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17
Q

acid + hydroxide/oxide =>

A

salt + water

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18
Q

acid + metal carbonate =>

A

salt + water + carbon dioxide

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19
Q

acid + metal =>

A

salt + hydrogen

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20
Q

Reaction for limewater

A

Ca(OH)2 + CO2 => CaCO3 + H2O

limewater + carbon dioxide => limestone [cloudy, milky] + water

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21
Q

Limestone Cycle

A

=> Limestone (CaCO3)
CO2. Burning or slaking. Heat 1100 degrees Celcius.

=> Quick lime CaO + CO2
Heat. Hydration or slaking.
Add water

=> Ca(OH)2 + H2O -> CaO [above] + CO2

=> Slaked lime. Ca(OH)2
+ H2O

=> back to

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22
Q

MS FORM

Limewater goes…
Chemical formula of limewater?
Limestone rock?

A

Limewater goes cloudy

Calcium hydroxide

Sedimentary rock

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23
Q

common uses of limestone (CaCO3)

A

building materials

manufacture of cement

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24
Q

common uses of CaO

A

wastewater treatment

neutralisation of acidic soil

25
Q

What is produced when calcium carbonate undergoes thermal decomposition?

A

Calcium oxide

26
Q

chemical name for slaked lime?

A

calcium hydroxide

27
Q

What is formed when excess carbon dioxide is bubbled through limewater?

A

calcium hydrogen carbonate

28
Q

Why does limewater appear milky when carbon dioxide is bubbled through it?

A

calcium carbonate is insoluble in water

29
Q

What is the correct balanced symbol equation for the formation of solid slaked lime?

a) CaO(s) + H2O(l) → 2CaOH2(s)

b) CaO(s) + H2O(l) → Ca(OH)2(aq)

c) CaO(s) + H2O(l) → Ca(OH)2(s

A

c)

30
Q

What is the correct balanced symbol equation for the formation of solid quick lime (CaO)?

a) CaCO3(s) → CaO(s) + H2O(l)

b) CaCO3(s) → CaO(s) + CO2(g)

c) CaO(s) + H2O(l) → Ca(OH)2(s)

A

b)
FORMATION so on the right

31
Q

What is the correct balanced symbol equation for the formation of solid limestone?

a) CaCO3(s) → CaO(s) + H2O(l)

b) Ca(OH)2 (aq) + CO2 (g) → CaCO3 (s)

c) CaCO3 (s) → CaO (s) + CO2 (g)

A

b)
formation so right side

32
Q

Flame tests of metal ions

  1. Lithium Li+
A

Red

33
Q

Sodium Na+

A

Yellow

34
Q

Potassium K+

A

Lilac

35
Q

Copper (II) (Cu2+)

A

Blue

36
Q

Calcium Ca2+

A

Orange

37
Q

Barium Ba2+

A

Light green

38
Q

Testing for anions - anion, test, test result

  1. Carbonate CO3 2-
A

Add dilute acid

Bubbles (CO2/milky)

39
Q
  1. Chloride Cl- in solution
A

Acidify with dilute nitric acid,

+ add aqueous silver nitrate

White ppt (AgCl)

40
Q
  1. Bromide Br- in solution
A

Acidify with dilute nitric acid,

+ add aqueous silver nitrate

Cream ppt (AgBr)

41
Q

Iodide I- in solution

A

Acidify with dilute nitric acid,

+ add aqueous silver nitrate

Yellow ppt (AgI)

42
Q

Nitrate NO3- in solution

A

Add aqueous sodium hydroxide, then aluminium foil; warm carefully

NH3
turns blue

43
Q

Sulfate SO4 2- in solution

A

Acidify, then add aqueous barium nitrate

White ppt (BaSO4)

44
Q

Sulfite SO3 2-

A

Add dilute hydrochloric acid, warm gently and test for the presence of sulfur dioxide

SO2
Decolourises

45
Q

Testing for aqueous cations - cation,

test effect of AQUEOUS SODIUM HYDROXIDE,

effect of aqueous ammonia

  1. Aluminium Al3+
A

White ppt

Soluble

46
Q
  1. Ammonium NH4+
A

No ppt

Produces NH3 on heating

47
Q
  1. Calcium Ca2+
A

White ppt

Insoluble

48
Q
  1. Chromium (III) Cr3+
A

Green ppt

Soluble

49
Q
  1. Copper (II) Cu2+
A

Light blue ppt

Insoluble

50
Q
  1. Iron (II) Fe2+
A

Green ppt

Insoluble

51
Q
  1. Iron (III) Fe3+
A

Red-brown ppt

Insoluble

52
Q

Zinc Zn2+

A

White ppt

Soluble

53
Q

Tests for gases - test, observation

  1. Ammonia NH3
A

Test: damp red litmus

Observation: litmus paper turn blue/purple

54
Q
  1. Carbon dioxide CO2
A

Test: bubble the gas through limewater

Observation: limewater goes milky/cloudy

55
Q

Chlorine Cl2

A

Test: damp blue litmus

Observation: litmus turns red or white/bleached

56
Q

Hydrogen H2

A

Test: splint

Observation: squeaky pop/flame flickered

57
Q

Oxygen O2

A

Test: glowing splint

Observation: lots of smoke, splint relit

58
Q

Sulfur dioxide SO2

A

Test: potassium permanganate paper

Observation: purple to colourless

Chemistry (N.A.) (7 decks)

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