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A level Chemistry 2 > Acids, Bases and Salts > Flashcards

Acids, Bases and Salts Flashcards

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1
Q

Definition of an acid

A

An acid releases H+ ions in aqueous solution. An acid is a proton donor.

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2
Q

Show dissociation of HCl and H2CO3

A

HCl (aq) –> H+ (aq) + Cl- (aq)

H2CO3 (aq) –> 2H+ (aq) + CO3 2- (aq)

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3
Q

Define a stong acid

A

A strong acid is fully dissociated in solution

It is not a reversible reaction

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4
Q

Define a weak acid

A

A weak acid is partially dissociated in solution.
Many are carboxylic or organic acid.
It is a reversible reaction

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5
Q

Show dissociation of CH3COOH

A

CH3COOH (aq) –> CH3COO- (aq) + H+ (aq)

reversible reaction

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6
Q

Define a base

A

Bases are proton acceptors

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7
Q

What are the different types of bases

A

Metal hydroxides
Metal oxides
Ammonia and organic amino compounds

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8
Q

Example of reaction of bases with acids:
NaOH +HCl
MgO + HCl
NH3 + H+

A

NaOH +HCl –> NaCl + H2O
MgO +2HCl –> MgCl2 + H2O
NH3 (aq) + H+ (aq)–> NH4+ (aq)

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9
Q

Neutralisation reaction

A

H+ + OH- –> H2O

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10
Q

Define an alkali

A

An alkali is a water soluble base that releases OH- ions in water e.g. NaOH, KOH, NH3

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11
Q

What happens when acid dissolves in water

A

The acid dissociates and the hydrogen ion is accepted by a water molecule so the water molecule is acting as a base.
H+ + H2O –> H3O+
(hydronium ion)

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12
Q

Water soluble metal oxide with water

A

water soluble metal oxide react with water to form aqueous hydroxides
If added to aqueous acid the hydroxide forms can react further to form water.

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13
Q

Water soluble metal hydroxide with water

A

Water soluble metal hydroxides dissolve and release hydrated OH- ions in water
NaOH (s) + aqua–> Na+ (aq) + OH- (aq)
Water is aqua because it is acting as a solvent and is not reacting chemically.

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14
Q

Define a salt

A

Salts are ionic compounds formed when H+ ions are replaced by metal ions or ammonium ions

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15
Q

Reactions of acids

A

Acid + Metal hydroxide –> Salt + Water
Acid + Metal oxide –> Salt + Water
Acid + Metal carbonate –> salt + CO2 + Water
Acid + Reactive metal –> salt + hydrogen

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16
Q

What happens when ionic compounds are added to water e.g NaCl

A

The ions leave the solid lattice and become separate hydrated ions . The polar water molecules surround the ions in the lattice and separate them form their compound. the separate ions are completely independent of each other so can react without affecting the other.

17
Q

Ions that form soluble compounds

A
  1. Group 1 ions
  2. Ammonium
  3. Nitrate
  4. Hydrogen carbonate
  5. Halides- except when with Ag+, Pb2 + or Hg2+
  6. Sulfate- except when with Ag+, Pb2 +, Ca2+, Sr2+, or Ba2+
18
Q

Ions that form insoluble compounds

A
  1. Oxide- except with group 1 melals , Ca2+, Ba2+
  2. Carbonate- except with group 1 ions or ammonium
  3. Phosphate- except with group 1 ions or ammonium
  4. Hydroxide- except with group 1 ions or ammonium, Ca2+, Mg 2+, Sr 2+, Ba2+
  5. Sulfide- except with group 1 ions or ammonium
  6. Chromate- except with group 1 ions or ammonium, Ca2 +, Mg 2+
19
Q

Test for Halide ions

A
  1. Add Ag+ ions
  2. Then dilute ammonia solution
  3. Then concentrated ammonia
    Results
    Chlorine- White precipitate forms, dissolves in dilute and concentrated ammonia
    Bromine- Cream precipitate forms, only dissolves in concentrated ammonia.
    Iodine- Yellow precipitate forms, doesn’t dissolve in either ammonia solutions.
20
Q

Test for carbonate ion

A

Add nitric acid
Results
Should see effervescence and gas produced should turn lime water cloudy.- CO2

21
Q

Test for sulfate ions

A

Add Ba 2+ ions as barium chloride or nitrate
Results
A white precipitate should form

22
Q

Test for ammonium

A

Add NaOH and warm it up
Results
Turn damp red litmus paper blue

23
Q

What are spectator ions

A

Ions that don’t undergo changes in a reaction and stay in solutions. Remove these in ionic equations

24
Q

Rules for ionic equations

A
  1. Remove spectator ions
  2. Don’t separate solids into ions
  3. Don’t separate covalent compounds into ions
  4. The atoms and the charge must be balanced

A level Chemistry 2 (22 decks)

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