Acid, Base and pH 1 Flashcards

1
Q

What is an Arrhenius base?

A
  • acid - produces (H+) hydrogen ion and anion in water
  • base - produces (HO-) hydroxide or hydroxyl ion and a cation in water
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2
Q

What is a Brønsted–Lowry Acid?

A

A proton (H+) donor

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3
Q

What is a Brønsted–Lowry base?

A

A proton (H+) acceptor

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4
Q

What is a Lewis acid?

A

species that accept electrons and it is termed as an electrophile, and are electron deficient species

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5
Q

What is a Lewis base?

A

species that donate electrons to a nucleus with an empty orbital and is a nucleophile

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6
Q

What are 2 Acid/Base reactions that occur in our body?

A

CO2 + H2O —> H2CO3
- CO2 transported in the blood reacts with water to form carbonic acid which is excreted by the lungs as a gas
Ca(OH)2 + 2HCl —> CaCl2 + 2H2O
- Antacid - Ca(OH)2 - neutralises
- Stomach acid - 2HCl

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7
Q

What are most drugs?

A
  • Weak Acids
  • Bases
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8
Q

What does an Acid produce in water?

A
  • hydrogen ion (H+)
  • an anion
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9
Q

What does a base produce in water?

A
  • hydroxide or hydroxyl ion (HO-)
  • a cation
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10
Q

What does a neutralisation reaction produce?

A

A salt

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11
Q

What is a salt?

A

Ionic compound made from an anion and cation

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12
Q

What is the limitation of strong acids and strong bases?

A

limited to Aqueous solutions

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13
Q

What occurs in an acid-base reaction?

A

a proton (H+) is transferred from an acid to a base

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14
Q

What are weak bases?

A

the conjugated base of strong acids - tends to accept protons

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15
Q

What is the Equilibrium constant?

A

k = Conc of products / conc of reactants

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16
Q

What is Ka?

A

Acidity Constant

17
Q

What do strong acids produce in terms of Ka?

A
  • large Ka
  • High H3O+ concentration
  • completely dissociated
18
Q

What do strong bases produce in terms of Ka?

A
  • small values for Ka
  • low H3O+ concentration
  • less dissociated
19
Q

What is the range of pKa values?

A

2-12

20
Q

What value of pKa shows a strong acid?

A

Less than 3

21
Q

What value of pKa shows a weak acid

A

Greater than 3

22
Q

What 5 factors influence acidity?

A
  • increasing electronegativity
  • increasing bond energy
  • inductive effects
  • Hybridisation effect
  • resonance/delocalisation effects
23
Q

How do electron donating and withdrawing groups influence acidity?

A

by destabilising or stabilising the conjugate base
- Withdrawing increases acidity
- donating decreases acidity

24
Q

What is pKb?

A

Conjugated base of the acid

25
Q

What is the pKw Equation?

A

pKw = pKa + pKb

26
Q

What value is the pKw constant?

A

14

27
Q

What is basicity?

A

The ability of a compound to use its nonbonding electrons to combine with a proton

28
Q

What influences basicity? 4 Examples

A
  • electronegativity
  • inductive effects
  • hybridisation effect
  • resonance/delocalisation effects
29
Q

What influence does electronegativity have on basicity?

A

Increasing electronegativity decreases basicity