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Chemistry > Acid-base reactions > Flashcards

Acid-base reactions Flashcards

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1
Q

What is an Arrhenius’ acid?

A

A substance that produces hydrogen ions (H+) or hydronium ions (H30+) when it dissolves in water

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2
Q

What is an Arrhenius’ base?

A

A substance that produces hydroxide ions (OH-) when it dissolves in water.

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3
Q

What is a Lowry-Bronsted acid?

A

A proton or H+ ion donor

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4
Q

What is a Lowry-Bronsted base?

A

A proton or H+ ion acceptor

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5
Q

What is an alkali?

A

A soluble base that contains hydroxide ions (OH-)which can be released into the solution

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6
Q

What is the difference in the ways that acids and bases ‘release’ their ions into water?

A

Acids ionise their ions in water, while bases dissociate their ions in water

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7
Q

Define ionise

A

The process whereby COVALENT compounds break up into ionic substances for the first time

(usually in the presence of water in these cases)

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8
Q

Define what it means when a substance dissociates its ions

A

The process whereby ionic compounds break up into their separate ions in the presence of water

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9
Q

Why is the H+ ion called a proton

A

It is essentially a Hydrogen atom that has lost its electron. As Hydrogen does no contain any neurons, there is effectively only a proton left in the + ions.

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10
Q

What are conjugate acid-base pairs?

A

Compounds that differ by the presence of 1 proton or H+ ion.

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11
Q

What do we call substances that can act as either acids or bases?

A

Amphiprotic or ampholytes

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12
Q

Define a strong acid

A

An acid which ionises completely in water

to form a high concentration of H3O+ ions

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13
Q

Give 3 examples of strong acids

A
  • Hydrochloric acid (HCl)
  • Suphuric acid (H2SO4)
  • Nitric acid (HNO3)
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14
Q

Define a weak acid

A

An acid which ionises incompletely in water

to forma low concentration of H3O+ ions

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15
Q

Give 2 examples of weak acids

A
  • ethanoic acid (CH3COOH)

- oxalic acid (C2 H2 O4)

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16
Q

Define a strong base

A

A strong base dissociates completely in water to form a high concentration of OH- ions

17
Q

Give 2 examples of strong bases

A
  • Sodium hydroxide (NaOH)

- Potassium hydroxide (KOH)

18
Q

Define a weak base

A

A weak base dissociates or ionises incompletely or partially in water to form a low concentration of OH- ions.

19
Q

Give 5 examples of weak bases

A
  • ammonia (NH3)
  • Potassium carbonate (K2CO3
  • Sodium hydrogen carbonate (NaHCO3)
  • calcium carbonate (CaCO3)
20
Q

What are concentrated acids or bases

And how are they different to dilute acids and bases

A

These acids/bases contain a large amount (#moles) of the acid/base in proportion to the volume of water.

Conversely small amount (#moles) for dilute acids/bases

21
Q

Define concentration

A

A ratio of the amount of solute to the volume of solvent in a solution

22
Q

In terms of conductivity what is the difference between strong and weak acids

Same applies to bases**

A

Strong acids have:

  • a high concentration of ions
  • because of their high degree of ionisation
  • Thus they will be good conductors of electricity

Lower degree of ionisation means lower concentration which means less conductivity

23
Q

Describe the reactivity of strong and weak acids and bases

A

Strong = react faster
Because there will be more ions present int he solution

Strong acids or bases will have higher degrees of ionisation or dissocitation (than weak acids or bases)

24
Q

Define a dilute acid

A

Contain small amount (#moles) of acid or base in proportion to volume of water

25
Q

Define hydrolysis

A

The reaction of a salt with water

26
Q

Equivalence point of a titration

Endpoint

A

The point at which the acid or base has completely reacted with the acid or base

The point where the indicator changes colour

27
Q

Auto ionization of water

A

The reaction of water with itself to form h30+

Chemistry (8 decks)

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