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chem unit 2 > 10A- acids and bases-Table 1 > Flashcards

10A- acids and bases-Table 1 Flashcards

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1
Q

Define acid

A

species that donates a proton, H+, during an acid-base reaction

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2
Q

Define acid-base reaction

A

chemical reaction where a proton, H+, is transferred between two
chemical species

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3
Q

Define alkali

A

a base that is soluble in water and neutralises acids

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4
Q

Define amphiprotic

A

species that can either donate or accept a
proton, H+

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5
Q

Define base

A

species that accepts a proton, H+, during an acid-base reaction and are a
group of substances that neutralise acids

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6
Q

Define Brønsted-Lowry
theory

A

definition of an acid as a chemical species
which donates a proton, H+,
to a base

Or

describes acid-base properties in terms of proton(H+) transfer

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7
Q

Define corrosive

A

A highly reactive substance that causes obvious damage to tissue

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8
Q

Define deprotonation

A

loss of a proton, H+, from an acid

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9
Q

Define diprotic

A

species that can donate up to two protons, H+, during ionisation

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10
Q

Define hydronium ion

A

positively charged chemical species with
molecular formula H3O+

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11
Q

Define hydroxide ion

A

negatively charged chemical species with
molecular formula OH−

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12
Q

Define ionisation

A

process by which a chemical species gains or loses an electron
to gain an electric charge

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13
Q

Define monoprotic

A

species that can only donate one proton, H+, during ionisation

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14
Q

Define neutralise

A

react with an acid or a base to produce water

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15
Q

Define polyprotic

A

species that donates multiple protons, H+, during ionisation

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16
Q

Define protonated water

A

alternate name for the hydronium ion, H3O+

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17
Q

Define strength

A

how readily an acid or base will donate or accept a proton, H+

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18
Q

Define triprotic

A

species that can donate up to three protons, H+, during ionisation

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19
Q

define caustic

A

Generally used to describe highly basic substances(looking at internet, looks like it can also be used to describe acids and is interchangeable with corrosive)(Check with choung)

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20
Q

What does the Bronsted-Lowry theory indicate about acids and bases

A

• An acid is a substance that donates a proton, H+
• A base is a substance that accepts a proton, H+
• An acid-base reaction involves the transfer of a proton from an acid to a base
• Acids and bases are corrosive substances.

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21
Q

What’s the difference between a hydronium ion and a hydroxide ion

A

Hydroxides is when water loses a hydrogen

Hydronium is when water gains a hydrogen

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22
Q

Is water required in all acid base reaction?

A

Yes, sometimes its not specified but some have aqueous solutions

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23
Q

Write the balanced equation for the acid-base reaction of hydrochloric acid, HCl, in aqueous solution

A

HCl(aq) + H2O(l) → H3O+(aq) + Cl−(aq)

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24
Q

How can a compound be both an acid and a base

A

It can be amphiprotic meaning that it donates and accepts protons in an acid base reaction like water

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25
Q

List some amphiprotic species

A

Water:H2O

hydrogen sulfate:HSO4-

Bicarbonate:HCO3-

Dihydrogen phosphate:H2PO4-

Hydrogen phosphate:HPO42-

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26
Q

What is giving up a proton known as

A

Deprotonation

27
Q

How can we classify types of acids

A

Monoprotic- only donate one proton

diprotic- donates two H+ ions

triprotic- can donate three H+ ions

polyprotic- can donate a H+ ion more than once

28
Q

List some monoprotic acids

A

Nitric acid:HNO3
hydrochloric acid:HCl
ethanoic acid:CH3COOH
ammonium:NH4

29
Q

List some diprotic acids

A

Sulfuric acid:H2SO4
carbonic acid:H2CO3
hydrogen sulfide:H2S
selenous acid:H2SeO3

30
Q

List some triprotic acids

A

Phosphoric acid:H3PO4
citric acid:C6H8O7
Boric acid:H3BO3
arsenic acid: H3AsO4

31
Q

What is a strong acid

A

A strong acid will readily undergo almost complete ionisation when added to water

essentially all acid molecules will donate their protons to form aqueous H+ ions

32
Q

What is a strong base

A

A strong base will readily accept H+ ions from an acid

33
Q

What is a weak acid

A

Does not readily give up its H+ ion in solution and only partially ionises.

34
Q

What are weak bases

A

Bases that don’t readily accept H+ ions

35
Q

List some strong acids

A

Sulfuric acid:H2SO4(aq) → HSO4−(aq) + H+(aq)

Hydrochloric acid: HCl(aq) → Cl−(aq) + H+(aq)

Nitric acid: HNO3(aq) → NO3−(aq) + H+(aq)

36
Q

List some weak acids

A

Ethanoic acid: CH3COOH(aq) CH3COO−(aq) + H+(aq)
Carbonic acid: H2CO3(aq) HCO3−(aq) + H+(aq)
Ammonium: NH4+(aq) NH3(aq) + H+(aq)

-H3PO4=phosphoric acid

37
Q

What are some strong bases

A

O2-
OH-
HPO4 2-

-NaOH=sodium hydroxide
-KOH=potassium hydroxide
-Ca(OH)2=calcium hydroxide

38
Q

Give an example of a weak base

A

NH3=Ammonia

NH3(aq) + H2O(l) NH4+(aq) + OH−(aq)

39
Q

Why do we use harpoon arrows

A

Harpoon/bidirectional arrows are used to indicate that the reactions don’t go to completion

40
Q

What compounds create a basic solution

A

Any compound that more or less completely dissociates to form ions, creates a basic solution

41
Q

What are some ionic compounds that function as strong bases as they readily dissociate to form OH- ions

A

NaOH, KOH, Ca(OH)2

act as a strong source of the base OH

42
Q

Compare strength and concentration

A

• Strength of an acid/base refers to what proportion of its molecules will donate a H+ ion/accept -> dependent on the identity of it

concentration depends on how many molecules there are to begin with- >Dependent on amount of particles/molecules

43
Q

What are some
common acids and their uses.

(probs don’t need
to know all but its just nice)

A

Common acids and
their uses=
-Hydrochloric
acid(HCl)=main component of stomach acid
-Sulfuric
acid(H2SO4)=used in car batteries
-nitric
acid(HNO3)=used to manufacture fertilisers, dyes and explosives
-ethanoic
acid(CH3COOH)=found in vinegar
-Carbonic
acid(H2CO3)=found in carbonated soft drinks
-phosphoric
acid(H3PO4)=used to manufacture fertiliser
-Ammonium(NH4)

44
Q

What are some characteristics of acids

A

-all acids taste
sour
-Acids=turn litmus
paper red
-acids=corrosive
-react with bases
-low pH
-acids conduct
electricity in water.

45
Q

What are some
common bases and their uses

A

Common bases and
their uses=
-sodium
hydroxide(NaOH)=used in drain and oven cleaners
-Ammonia(HN3)=used
in household cleaners, fertilisers and explosives.
-calcium
hydroxide(Ca(OH)2)=used in garden lime to adjust soil pH.
-magnesium
hydroxide(Mg(OH)2)=key ingredient in some antacids
-sodium
carbonate(Na2CO3)=used to manufacture washing powder.
-Oxide
-Potassium
hydroxide

46
Q

What are sone
characteristics of acids

A

-all bases taste
bitter
-Bases=litmus to
blue
-react with acids
-high pH
-corrosive(known
as caustic for bases)
-feel slippery

47
Q

What is a
proton/hydrogen ion in a solution represented by

A

:hydronium
ion(H3O+)
:hydrogen ion(H+)

48
Q

What is the
difference between caustic and corrosive

A

Caustic
and corrosive both mean A
highly reactive substance that causes obvious damage to tissue

A
difference between corrosive and caustic is that caustic is utilised
generally to describe bases, where as corrosive is used to describe acids.

49
Q

What
arrow is used to show a reaction with a strong acid
or base

A

-Full
arow → is used to show a
reaction with a strong acid or base

50
Q

What
arrow is used to show a reaction with a weak acid or
base

A

-Equilibrium Arrow ⇌ is used to
show a reaction with a weak base or acid

51
Q

How can you
determine if a molecule is amphiprotic

A

-all amphiprotic
species have a negative charge=this allows it to give a charge, as well as
except a charge
-All amphiprotic
species also have 1 or 2 extra hydrogens that it is able to donate.

52
Q

Difference between
strong acids/bases and weak acids/bases

A

Strong
acids/bases= will ionise readily= virtually no unreacted acid molecules
Weak
acids/bases=will ionise a small proportion= large number of unreacted acid
molecules

53
Q

Define
strength(adj.), in terms of strength of an acid or base

A

-strength(adj.)=Tendency to dissociate

-in context of
acids and bases= ‘strong’ and ‘weak’= refer to the relative tendency to
accept or donate protons.

54
Q

Define
concentration(adj.)

A

-concentration(adj.)=the amount of acid or
base ions dissolved in a solvent

55
Q

Difference between
concentration and strength of an acid

A

:strenght
and concentration are two separate properties=
-strength=refers to a substances willingness
to ionise
-concentration=refers to how much of a
substance is present within a solution

56
Q

What will happen
to a
1)strong dilute
solution
2)strong
concentrated solution
3)weak dilute
solution
4)weak
concentrated solution

A

1)strong
dilute solution=will fully ionise
2)strong
concentrated solution=will fully ionise
3)weak
dilute solution=no reacted ions
4)weak
concentrated solution=unionised

57
Q

What is=
-HCl’s conjugate
-waters conjugate

A

HCl(aq){acid}+H2O(l){base}
→ H3O+(aq) + Cl-(aq)

-HCl’s conjugate
base is a chloride ion
-waters conjugate
acid is hydronium ion

58
Q

What is=
-NH3’s conjugate
-H2O’s conjugate

A

NH3(aq){acid} +
H2O(l){base} → NH4+(aq) + OH-(aq)

-NH3’s conjugate
base is ammonium ion
-H2O’s conjugate
acid is hydroxide ion

59
Q

What is a
conjugate

A

-Oxford
dictionary=(of an acid or base) related to the corresponding base or acid by
loss or gain of a proton.

-In acid and base
conjugate pair=the acid always has one hydrogen extra in comparison to its
base conjugate.

-In base and acid
conjugate pair=the base always has one hydrogen less in comparison to its
acid conjugate.

-Explanation of
conjugate acid and base=
A
conjugate acid isthe product that is different from a base by
one proton.
Examples of conjugate acids include water (base) reacting with an acid to
form the hydronium ion (conjugate acid), and ammonia (base) reacting with an
acid to form the ammonium ion (conjugate acid).

60
Q

Are the conjugate
bases of strong acids always weak or always strong.

A

Conjugate bases of
all strong acids will be weak

-I don’t think
this is the same pattern for weak bases, weak acids and strong bases. This
only occurs for the conjugate bases of strong acids.(check with Choung but
this is what vid says)

61
Q

Patterns I have
noticed in determining whether a base is strong or weak and whether and acid
is strong or weak, but this may not be always true(FELIX OBSERVES)

A

Strong acids=
:Generally have
extra H, and are not carboxylic, and some have hydroxyl groups(sulfuric acid)
:they are
generally covalently bonded molecules

Weak acids=
:Generally
carboxylic acids
:Generally
covalently bonded molecules

Strong bases=
:Have ionic bonded
hydroxides
:generally ionic

Weak bases=
:Just missing a
hydrogen
:Hydrogen
ionically attracted with weak base
:e.g. Is ammonia

62
Q

What are the
functional groups acids normally have, but this may not be always true(FELIX
OBSERVES)

A

Acids generally
have=
:carboxyl group
:hydroxyl group
:has hydrogens

63
Q

What are the
functional groups bases normally have, but this may not be always true(FELIX
OBSERVES)

A

Bases generally
have=
:hydroxyl groups
:carbonate
:or can fit in
hydrogens

64
Q

What is the
difference between hydroxyl and hydroxy(I THINK .THIS IS FROM INTERNET)

A

Hydroxyl refers to
the hydroxyl radical (OH-) only while the functional group OH is called
hydroxy group.

chem unit 2 (7 decks)

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