2.1.4: Acids Flashcards

1
Q

Weak acid:

A
  • Partially dissociates

* e.g. CH₃COOH ⇌CH₃COO⁻ + H⁺

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2
Q

Strong acid:

A
  • Fully dissociates

* e.g. HCl ⟶ H⁺ + Cl⁻

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3
Q

Bronsted-Lowry base

A

A proton acceptor

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4
Q

Bronsted-Lowry acid

A

A proton (H⁺) donor

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5
Q

What is a monoprotic acid?

A

Donates 1 proton

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6
Q

Typical properties of acids

A
  • Usually taste sour
  • pH less than 7
  • Aqueous solutions of acids contain H⁺ ions
  • Acid = proton (H⁺) donor
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7
Q

Ionic equation for neutralisation reaction

A

H⁺ + OH⁻ ⟶ H₂O

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8
Q

Acid + base

A

Acid + base ⟶ salt + water

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9
Q

Acid + carbonate

A

Acid + carbonate ⟶ salt + water + carbon dioxide

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10
Q

Acid + metal

A

Acid + metal ⟶ salt + hydrogen

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11
Q

Acid + metal oxide

A

Acid + metal oxide ⟶ salt + water

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12
Q

Acid + metal hydroxide

A

Acid + metal hydroxide ⟶ salt + water

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13
Q

Conjugate base

A

The base that accepts the proton donated by the acid.

e.g. Cl⁻ in HCl

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14
Q

Concentrated acid

A

Fewer water molecules per unit volume than a dilute acid.

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15
Q

Acids release __ ions into solution

A

H⁺

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16
Q

Alkalis release __ ions into solution

A

OH⁻

17
Q

Alkali

A

A soluble base

18
Q

Salt

A

An ionic compound

19
Q

How is a salt formed?

A

By replacing the H⁺ ions in an acid with metal ions.

20
Q

Hydrated salts

A

Contain water molecules in their crystal structure

Given as .xH₂O

21
Q

Anhydrous

A

Opposite of hydrated; salts that do not contain water molecules in their crystal structure.

22
Q

What is the water in a hydrated salt known as?

A

Water of crystallisation

23
Q

Molecules that can either donate or accept a proton depending on the circumstances

A

‘Amphiprotic’

24
Q

Amphiprotic

A

Molecules that can either donate or accept a proton depending on the circumstances