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U1&2 Chemistry > U2 AOS1 Chapter 10 A&B > Flashcards

U2 AOS1 Chapter 10 A&B Flashcards

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1
Q

acid base reaction

A

H+ is transferred from the acid to the base

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1
Q

acid

A

species that donates a proton during an acid base reaction

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2
Q

alkali

A

water-soluble base that neutralises acids

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3
Q

amphiprotic

A

A species that can either accept or donate a proton.

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4
Q

base

A

species that accepts a proton

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5
Q

Bronsted Lowry theory

A

defines an acid as a hydrogen-ion donor, and a base as a hydrogen-ion acceptor

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6
Q

corrosive

A

Highly reactive substance that causes obvious damage to other substances

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7
Q

deprotonation

A

loss of a proton; forming of an acid

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8
Q

diprotic

A

an acid that can donate up to two protons

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9
Q

hydronium ion

A

positive ion, H30+

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10
Q

hydroxide ion

A

negative ion, OH-

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11
Q

monoprotic

A

An acid that can only donate one proton

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12
Q

neutralise

A

react with acid or base to produce water

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13
Q

polyprotic

A

an acid that can donate multiple protons during ionisation

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14
Q

protonated water

A

hydronium, H3O+

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15
Q

triprotic

A

an acid able to donate up to three protons

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16
Q

strength

A

how readily an acid or base ionises

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17
Q

properties of acids

A
  1. sour
  2. molucular
  3. poorly conducts electricity
  4. corrosive
  5. dissolves in water
  6. H+ ions
  7. red litmus stays red, blue litmus turns red
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18
Q

properties of bases

A
  1. bitter
  2. ionic
  3. conducts electricity
  4. can be corrosive
  5. dissolves in water
  6. red litmus turns blue, blue litmus stays blue
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19
Q

acid equation eg.

A

HNO3 + H2O <-> NO3- +H3O+

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20
Q

base equation (water) eg.

A

NH3 + H2O <-> NH4+ + OH-

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21
Q

base equation (no water) eg.

A

NaOH <-> Na+ + OH-

22
Q

conjugate acid base pair

A

two species that differ by a single proton eg. NH3(aq) <-> NH4+

23
Q

amphiprotic species eg

A

water (H2O) bicarbonate (HCO3-) hydrogen sulfate (HSO4-), hydrogen phosphate (HPO42-)

24
Q

polyprotic substance conditions

A

depends on no. of acidic hydrogens (not total H) eg. CH3COOH (one disassociates)

25
Q

weak acid/base

A
  1. only partially ionises in water
  2. concentration of acid/base does not indicate concentration of hydronium/hydroxide ions
  3. equilibrium arrow
26
Q

strong acid/base

A
  1. ionises completely in water
  2. concentration of acid/base is the same as the concentration of hydronium/hydroxide ions
  3. no equilibrium arrow
27
Q

strong acid eg

A

sulfuric H2SO4, hydrochloric HCl, nitric HNO3

28
Q

weak acid eg.

A

ethanoic CH3COOH, carbonic H2CO3, ammonium NH4+,

29
Q

SHNECA

A

sulfuric (H₂SO₄), Hydrochloric (HCl), nitric (HNO₃), ethanoic (CH₃COOH), carbonic (H₂CO₃), ammonia (CHOOH)

30
Q

concentration

A

quantity of solute present in a given quantity of solution (molarity (M) = mol/L)

31
Q

what makes an acid weak? Why can’t it ionise completely?

A

with each depronotonation, harder for H+ to escape negative charge = decreasing distribution of ions

32
Q

antacid

A

weak base used to neutralise stomach acid

33
Q

heartburn

A

burning sensation produced by acid reflux into the esophagus

34
Q

indigestion

A

symptoms resulting from difficulty in digesting food

35
Q

neautralisation reaction

A

reaction between an acid and a base to form a salt and water

36
Q

ulcer

A

break in the lining of an organ ie stomach

37
Q

metal carbonate

A

base formed from metal cation and carbonate ions (CO3^2-)

38
Q

acid + metal carbonate

A

salt + water + carbon dioxide

39
Q

insoluble metal carbonate

A

remain in solid form eg. MgCO3, CaCO3

40
Q

metal hydrogen carbonate

A

containing metal cation and bicarbonate ion (HCO3)

41
Q

acid + metal hydrogen carbonate

A

salt + water + carbon dioxide

42
Q

spectator ion

A

an ion that appears on both sides of an equation and is in an aqueous state

43
Q

metal hydroxide

A

metal cation and hydroxide ions (OH-)

44
Q

acid + metal hydroxide

A

salt + water

45
Q

acid + metal

A

salt + hydrogen gas

46
Q

acid + metal oxide

A

salt + water

47
Q

acidic non metal oxide + base

A

salt + water

48
Q

neutralisation reaction

A

acid + base = salt + water

49
Q

antacid side effects

A

Mg(OH2) = laxative, Al(OH)3 = constipation, NaHCO3, CaCO3 = bloating, burping, flatulence

50
Q

why are calcium hydroxide and sodium hydroxide not used as antacids?

A

antacids are weak, Ca(OH)2 and NaOH are strong bases

51
Q

g to mg conversion

A

1 g = 1000 mg

52
Q

acid vs conjugate base (strength)

A

if acid is strong, base is weak

U1&2 Chemistry (10 decks)

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