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LC Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Arrhenius definition of an acid

A

An acid is a substance that dissociates in water to produce H+ ions

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2
Q

Arrhenius definition of A base

A

Is a substance that dissociates in water to form OH- ions

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3
Q

Arrhenius definition of A strong acid

A

A substance that almost completely dissociates in water to give H ions

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4
Q

Arrhenius definition of A weak acid

A

A substance that only slightly dissociates in water to give H ions

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5
Q

Arrhenius definition of a strong base

A

A substance that almost completely dissociates in water to form OH ions

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6
Q

Arrhenius definition of A weak base

A

Substance that only slightly dissociates in water to give hydroxide ions

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7
Q

Brønsted-Lowry definition of an acid

A

An acid is a proton donor

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8
Q

Brønsted-Lowry definition of A base

A

A proton acceptor

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9
Q

Brønsted-Lowry definition of Strong acid

A

A good proton donor

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10
Q

Brønsted-Lowry definition of A weak acid

A

Poor proton donor

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11
Q

Brønsted-Lowry definition of A strong base

A

Good proton acceptor

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12
Q

Brønsted-Lowry definition of A weak base

A

Poor proton acceptor

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13
Q

What is an alkali

A

A base that is solvable in water

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14
Q

What is a proton otherwise known as

A

A H+ ion

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15
Q

What does the Equilibrium symbol mean?

A

Reaction is going in both directions Ie you cannot know moles from the balanced equation

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16
Q

What is a monoprotic/basic acid

A

An acid that dissociates to give one proton

17
Q

What is a diprotic/basic acids

A

An acid that dissociates to give 2 protons

18
Q

Give an example of a monoprotic balanced equation

A

HCl=H+ + Cl-

19
Q

Give an example of a diprotic balanced equation

A

H2SO4 + H2O = H3O+ + HSO4-

20
Q

What are the limitations to Arrhenius’ theory of acids and bases

A

H+ ions do not exist on their own in solution. They form the H3O+ ion

Arrhenius’ definitions are restricted to aqueous solutions. Water is not the only solvent

NH3 cannot be considered a base

21
Q

Compare Arrhenius and Brønsted-Lowry

A

Arrhenius:
-Theory is restricted to only aqueous solutions
-bases produce OH- ions in water
- does not take hydronium ion formation into account

Brønsted-Lowry:
-can involve reactions that occur in the gaseous state
- not all bases produces OH- ions for example NH3
- takes hydronium ion formation into account

22
Q

What does amphoteric mean

A

Behave as either an acid or a base

23
Q

Under what circumstances do acids become conjugate bases?

A

When it donates a proton

24
Q

Under what circumstances does a base become a conjugate acid

A

Accepts a proton

25
Q

What is a conjugate base pair

A

Any pair consisting of an acid and a base that differ by a proton

26
Q

How to find the conjugate base

A

Decrees no of H by 1
Decrease charge by 1

27
Q

How to find conjugate acid

A

Increase no of H by 1
Increase charge by 1

28
Q

What does a strong acid have

A

Weak conjugate base

29
Q

What does a weak acid have

A

A strong conjugate base

30
Q

Why do strong acids have weak conjugate bases

A

Strong acids fully disassociate In water and it is unlikely for a reaction to go in the reverse direction thus it is a weak base

31
Q

Write a balanced equation to show how acid dissociates in water

A

Acid + water = weak base + acid

32
Q

Neutralisation

A

A reaction between an acid and a base, forming a salt and a water

33
Q

Eg of a neutralisation balanced equation

A

NaOH+HCl ->NaCl + H2O

34
Q

What is a salt

A

A substances formed when the H+ ion from an acid is replaced by a metal or ammonium ion

35
Q

Give an example of a balanced equation of a salt

A

NaOH + HCl -> NaCl + H2O

36
Q

Give 2 examples of a neutralisation reaction

A

Agriculture- if soil is too acidic lime is spread on soil to increase pH. Some crops do not grow well in acidic soil
CaO + H2O -> Ca(OH)2

Environmental- In areas where acid rain is a problem limestone is added to lakes to increase pH
H2SO4 + CaCO3 -> CaSO4 + H2O + CO2

LC Chemistry (22 decks)

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