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Chemistry Revision > Physical Chemistry (Acids, Alkalis, Salts, Energetics, Rates Of Reaction, Equilibria) > Flashcards

Physical Chemistry (Acids, Alkalis, Salts, Energetics, Rates Of Reaction, Equilibria) Flashcards

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1
Q

Universal indicator:
Acid:
Neutral:
Alkali:

A 
Strongly acidic: Red
Weakly acidic: Orange
Neutral: Green
Weakly alkali: Blue
Strongly alkali: Purple
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2
Q

Litmus paper:
Acid:
Neutral:
Alkali:

A

Acid: Red
Neutral: Purple
Alkali: Blue

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3
Q

Phenolphthalein:
Acid:
Alkali:

A

Acid: Colourless
Alkali: Pink

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4
Q

Methyl Orange:
Acid:
Alkali:

A

Acid: Red
Alkali: Yellow

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5
Q

Ph 0 =

A

Strongly acidic

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6
Q

Ph 14 =

A

Strongly acidic

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7
Q

An acid is a source of ____________ ions

A

Hydrogen ions (H+)

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8
Q

An alkali is a source of ____________ ions

A

Hydroxide ions (OH-)

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9
Q

The reaction between an acid and an alkali (or an acid and a base) is known as:

A

Neutralisation

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10
Q

Acid + Base–>

A

Acid + Base–> Salt + Water

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11
Q

Acid + Metal Oxide–>

A

Acid + Metal Oxide–> Salt + Water

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12
Q

Acid +Metal Carbonate –>

A

Acid +Metal Carbonate –> Salt + Water + Carbon dioxide

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13
Q

If the acid is hydrochloric acid, the salt will be a metal ___________

A

Chloride

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14
Q

If the acid is sulfuric acid, the salt will be a metal ___________

A

Sulfate

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15
Q

If the acid is nitric acid, the salt will be a metal ___________

A

Nitrate

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16
Q

Everything is soluble except for:

A

Carbonates (Except for sodium potassium and ammonium)
Barium sulfate
Calcium sulfate
Silver chloride

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17
Q

How do you make a soluble salt using acids

A

Add an insoluble base

18
Q

Describe making a soluble salt using acids + insoluble bases

A

Add the insoluble base to the acid. The solid will dissolve. The acid had neutralised when the excess solid sinks to the bottom of the flask.
You can then filter out the excess solid to get the salt solution.
For pure, sold crystals of salt, evaporate off the water.

19
Q

How do you make soluble salts from an alkali

A

Titrations

20
Q

How do you make insoluble salts

A

Precipitation reaction

21
Q

Describe a precipitation reaction:

A

Pick two solutions with the ions you need and mix them

22
Q

How do you do a titration

A
  1. Add (25cm3 of) alkali to a conical flask alongside indicator
  2. Meanwhile, fill a burette with acid (below eye level)
  3. Add the acid to the alkali (using a burette)
  4. The indicator will change colour when neutralisation takes place
  5. Record the volume of acid used to neutralise the alkali
  6. Repeat
23
Q

What four things does a rate of reaction depend on:

A

Temperature
Concentration (pressure)
Catalyst
Size of particles (surface area)

24
Q

Rate of reaction equation

A

Rate of reaction = amount of product formed (or reactant used) / Time

25
Q

What are the 3 ways the speed of reaction can be measure

A

Precipitation
Change in mass
Volume of gas given off

26
Q

How does a catalyst speed up a reaction

A

By providing an alternative pathway with lower activation energy

27
Q

What is activation energy

A

The minimum energy needed by reacting particles for the reaction to occur

28
Q

Chemical reactions in which heat is given out are known as ______________

A

Exothermic

29
Q

Chemical reactions in which heat is taken in are known as ______________

A

Endothermic

30
Q

Energy is _____________ to break existing bonds - so bond breaking is an _____________ process

A

Supplied

Endothermic

31
Q

Energy is _____________ when new bonds are formed - so bond formation is an _____________ process

A

Released

Exothermic

32
Q

If the value of enthalpy change is negative, the reaction is ______thermic

A

Exothermic

33
Q

If the value of enthalpy change is positive, the reaction _____thermic

A

Endothermic

34
Q

In an exothermic energy level diagram, the reactants are __________ the products

A

Above

35
Q

In an endothermic energy level diagram, the reactants are __________ the products

A

Below

36
Q

What is a reversible reaction

A

Where the products of the reactions can themselves react to produce the original reactants

37
Q

Describe the thermal decomposition of ammonium chloride

A

When heated, ammonium chloride breaks down into ammonia and hydrogen chloride. When the ammonia and hydrogen chloride cool, they re-form to make ammonium chloride

38
Q

What does equilibrium mean

A

That the relative quantities of reactants and products will reach a certain balance and stay there

39
Q

In a reversible reaction, the position of equilibrium depends on the ____________ and ____________ of the reacting mixture

A

Temperature and pressure

40
Q

What is the effect of increasing temperature on equilibrium.

What is the effect of decreasing temperature on equilibrium

A

If you increase the temperature, endothermic reaction will increase (to use up extra heat)
If you decrease the temperature, exothermic reaction will increase (to give out more heat)

41
Q

What is the effect of increasing pressure on equilibrium

What is the effect of decreasing pressure on equilibrium

A

If you increase the pressure, it will encourage the reaction which produces fewer molecules of gas
If you decrease the pressure, it will encourage the reaction which produces more molecules of gas

42
Q

What is dynamic equilibrium

A

The reactions are still taking place in both directions, but the overall effect is nil because they cancel each other out

Chemistry Revision (9 decks)

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