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Chemistry GCSE > Types Of Chemical Reactions > Flashcards

Types Of Chemical Reactions Flashcards

1
Q

What is a neutralisation reaction

A

Tje reaction between an acid and a base that produces a neutral solution

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2
Q

What is an acid

A

A substance, that when dissolved in water, releases H+ ions

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3
Q

What is the deifference between a base and alkali

A

A base is a substance that neutralises an acid, whereas alkalis are also able to neutralise acids, but release OH- ions when dissolved in water

Alkali - release OH- ions in water when dissolved
Base - neutralise acid

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4
Q

What is an alkali

A

A substance, that when dissolved in water realises OH- ions

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5
Q

What is produced when an acid reacts with a base

A

Produced a SALT + WATER

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6
Q

What happens when an acid reacts with a metal

A

Produces SALT + hydrogen

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7
Q

What happens when an acid reacts with a metal carbonate

A

produces SALT + WATER + CO2

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8
Q

How to find what salt is created?

A

First element of alkali plus last element of acid

hydroCHLORIC acid + SODIUM hydroxide —> SODIUM CHLORIDE

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9
Q

Why is universal indicator not used as indicator

A
  • Universal indicator shows gradual color changes through a range of colours which making it hard to detect precise endpoints.
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10
Q

What is the shape of a pH graph curve

A

A mirrored S shape

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11
Q

What is the definition of a concentrated acid

A

It is a substance which has a high ratio of acid to volume of solution

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12
Q

What is the definition of a dilute acid

A

An substance which has a low ratio of acid to volume of solute

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13
Q

How do you change how can concentrated an acid is

A

By changing the volume of water it is dissolved in. More water means that it is less concentrated and vies versa

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14
Q

What is the definition of a strong acid

A

A strong acid is an acid which fully dissociates in water
— (all of the molecules get split up into their ions)

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15
Q

What is the definition of a weak acid

A

An acid which only partially dissociates in water
—(only some particles split into ions)

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16
Q

What can weak acids do

A

Weak acids are reversible, meaning that they can split and join back together

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17
Q

What is pH

A

pH is the measure of the concentration of H+ ions in a solution

18
Q

What does it mean by a weak, concentrated acid

A

-> almost all particles are bonded tightened
-> BUT there are a lot of them, meaning that they can be corrosive

19
Q

What does it by mean by weak, dilute acid

A

-> very few particles are dissociated
-> and there is a low ratio acid particles to volume of solute

20
Q

What is the meaning of strong, concentrated acid

A

-> all of the moleucles are dissociated
-> there are a lot of these ions present
most corrosive

21
Q

What does it mean by strong, dilute acid

A

-> all molecules are dissociated
-> BUT, there are not that many of them, meaning it is not as dangerous

22
Q

What is the process of oxidation in terms of oxygen

A

Gain of oxygen

23
Q

What happens to the pH when a metal is added to a sample of acid

A

The pH will be below 7, and the magnesium will fizz

24
Q

What happens when metal is added to a sample of an alkali

A

-> the pH remains above 7
-> no reaction with magnesium

25
Q

What happens to the pH when a metal carbonate is added to an acid

A

The pH increases a lot more than with just a metal, which increases very slightly

26
Q

Why is it different when a metal and metal carbonate are dissolved in water

A

In a metal carbonate, the H+ ions react to form H20, making it have a much higher pH. In just the metal, the H+ ions only reduce to form H2 atoms, meaning it only increases slightly

27
Q

The reaction of methane and oxygen produces heat. Explain why (3 marks)

A

The bonds breaking is endothermic
The bonds being made is exothermic
More energy is given out than taken in meaning that the reaction is exothermic

28
Q

What does a reducing agent do in terms of electrons

A

It donates electrons to the +ve ions

29
Q

What is a piece of equipment that a student could use to test the pH of a substance

A

pH probe

30
Q

How to use a pH probe

A
  • wash the probe
  • put it in the solution
31
Q

The student concluded that the higher the reactivity, the higher the temp rise. How could she check this

A

-> use different masses
-> range of metals

32
Q

What is reduction in terms of OXYGEN

A

it is the LOSS of oxygen

Oxygen is removed from the oxidising agent and given to the reducing agent

33
Q

Describe the relationship between the number of carbon atoms in the molecule and it’s boiling point

A

-> as the molecules increase, so does the boing point
->because of the greater intermolecular forces between them

34
Q

How to make a dry sample of a salt

A

-> have an excess of the base/alkali
-> whilst reacting, heat them
-> filter excess base/alkali used from the solution
-> evaporate most of the water from the solution of water and Salt
-> leave it to dry in an oven

35
Q

How can you tell in titration when the alkali is just neutralised

A

-> One drop makes the colour change
-> goes from blue to red

36
Q

What does a white precipitate mean

A

That the product has an ion in it, most commonly. Sulfate, chlorine, carbonate, nitrate

37
Q

Which ions from precipitates

A

Sulfate ions + barium
Chlorine ions + silver

38
Q

Describe how a sample of solid ammonium sulfate is prepared in a laboratory.
Explain why this method is not suitable to be used industrially.

A

-> titre ammonia against sulphuric acid to get exact amounts to have them fully react
-> add the correct volumes without and indicator solution
-> slowly evaporate the solution over a hot bath
-> the reason it is not industrially used is that it is very hard to steam it at a large scale

39
Q

What to do when describing a neutralisation reaction

A

Write the names of the products and the names of the reactants

40
Q

What apparatus is used to measure volume of gas produced in a reaction

A

-> gas syringe
-> beaker / flask

41
Q

What is on the end of every alkali and what is on the end of every acid

A

alkali = hydroxide
Acid = Always has H at the beginning of chemical formula

42
Q

Write the ionic equation for neutralisation

A

(H+) + (OH-) —> H2O

Chemistry GCSE (15 decks)

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