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

10A- acids and bases-Table 1 Flashcards

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
List some amphiprotic species
Water:H2O hydrogen sulfate:HSO4- Bicarbonate:HCO3- Dihydrogen phosphate:H2PO4- Hydrogen phosphate:HPO42-
26
What is giving up a proton known as
Deprotonation
27
How can we classify types of acids
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
List some monoprotic acids
Nitric acid:HNO3 hydrochloric acid:HCl ethanoic acid:CH3COOH ammonium:NH4
29
List some diprotic acids
Sulfuric acid:H2SO4 carbonic acid:H2CO3 hydrogen sulfide:H2S selenous acid:H2SeO3
30
List some triprotic acids
Phosphoric acid:H3PO4 citric acid:C6H8O7 Boric acid:H3BO3 arsenic acid: H3AsO4
31
What is a strong acid
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
What is a strong base
A strong base will readily accept H+ ions from an acid
33
What is a weak acid
Does not readily give up its H+ ion in solution and only partially ionises.
34
What are weak bases
Bases that don't readily accept H+ ions
35
List some strong acids
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
List some weak acids
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
What are some strong bases
O2- OH- HPO4 2- -NaOH=sodium hydroxide -KOH=potassium hydroxide -Ca(OH)2=calcium hydroxide
38
Give an example of a weak base
NH3=Ammonia NH3(aq) + H2O(l) NH4+(aq) + OH−(aq)
39
Why do we use harpoon arrows
Harpoon/bidirectional arrows are used to indicate that the reactions don't go to completion
40
What compounds create a basic solution
Any compound that more or less completely dissociates to form ions, creates a basic solution
41
What are some ionic compounds that function as strong bases as they readily dissociate to form OH- ions
NaOH, KOH, Ca(OH)2 act as a strong source of the base OH
42
Compare strength and concentration
• 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
What are some common acids and their uses.   (probs don't need to know all but its just nice)
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
What are some characteristics of acids
-all acids taste sour -Acids=turn litmus paper red -acids=corrosive -react with bases -low pH -acids conduct electricity in water.
45
What are some common bases and their uses
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
What are sone characteristics of acids
-all bases taste bitter -Bases=litmus to blue -react with acids -high pH -corrosive(known as caustic for bases) -feel slippery
47
What is a proton/hydrogen ion in a solution represented by
:hydronium ion(H3O+) :hydrogen ion(H+)
48
What is the difference between caustic and corrosive
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
What arrow is used to show a reaction with a strong acid or base
-Full arow → is used to show a reaction with a strong acid or base
50
What arrow is used to show a reaction with a weak acid or base
-Equilibrium Arrow ⇌ is used to show a reaction with a weak base or acid
51
How can you determine if a molecule is amphiprotic
-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
Difference between strong acids/bases and weak acids/bases
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
Define strength(adj.), in terms of strength of an acid or base
-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
Define concentration(adj.)
-concentration(adj.)=the amount of acid or base ions dissolved in a solvent
55
Difference between concentration and strength of an acid
: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
What will happen to a 1)strong dilute solution 2)strong concentrated solution 3)weak dilute solution 4)weak concentrated solution
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
What is= -HCl's conjugate -waters conjugate
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
What is= -NH3's conjugate -H2O's conjugate
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
What is a conjugate
-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 is the 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
Are the conjugate bases of strong acids always weak or always strong.
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
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)
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
What are the functional groups acids normally have, but this may not be always true(FELIX OBSERVES)
Acids generally have= :carboxyl group :hydroxyl group :has hydrogens
63
What are the functional groups bases normally have, but this may not be always true(FELIX OBSERVES)
Bases generally have= :hydroxyl groups :carbonate :or can fit in hydrogens
64
What is the difference between hydroxyl and hydroxy(I THINK .THIS IS FROM INTERNET)
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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