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GCSE WJEC Chemistry > Topic 8 - Acids, Bases and Salts > Flashcards

Topic 8 - Acids, Bases and Salts Flashcards

1
Q

What is a base?

A

Bases are proton (H+) acceptors.

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2
Q

Is a base soluble?

A

Bases can either be soluble or insoluble in water. A soluble base is an alkali.

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3
Q

What is an alkali?

A

Soluble bases are known as alkalis, which are substances that release hydroxide (OH-) ions in aqueous solutions.

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4
Q

Examples of alkalis?

A

Alkalis are typically metal hydroxides.

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5
Q

Examples of bases?

A

Bases are typically metal oxides and metal carbonates.

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6
Q

What is the pH scale?

A

The pH scale is used to measure a substance’s ability to donate or accept a proton (H+).

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7
Q

What is an acid?

A

Acids are proton (H+) donors.

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8
Q

Examples of acids?

A

Nitric acid, sulfuric acid, hydrochloric acid

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9
Q

What do acids form in water?

A

Acids form hydrogen (H+) ions when they dissolve in water.

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10
Q

What do bases form in water?

A

Bases form hydroxide (OH-) ions when they dissolve in water.

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11
Q

What pH is acidic?

A

<7

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12
Q

What pH is neutral?

A

7

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13
Q

What pH is basic?

A

> 7

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14
Q

What is a strong acid?

A

An acid with a high ability to donate H+ ions and fully ionises in water e.g. Hydrochloric Acid.

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15
Q

What is a weak acid?

A

An acid with a low ability to donate H+ ions that doesn’t fully ionise in water e.g. Ethanoic Acid.

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16
Q

What is a strong base?

A

A base with a high ability to accept H+ ions that fully ionises in aqueous solutions e.g. Sodium/Potassium Hydroxide.

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17
Q

What is a weak base?

A

A base with a low ability to accept H+ ions that doesn’t fully ionise in aqueous solutions e.g. Ammonia.

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18
Q

What is ionisation?

A

Ionisation is the forming of ions, usually when reacting with water.

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19
Q

What is a concentrated acid?

A

Concentrated acids have a high number of moles of H+ ions per unit volume.

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20
Q

What is a dilute acid?

A

Dilute acids have a low number of moles of H+ ions per unit volume.

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21
Q

What is a concentrated base?

A

Concentrated bases have a high number of moles of OH- ions per unit volume.

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22
Q

What is a dilute base?

A

Dilute bases have a low number of moles of OH- ions per unit volume.

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23
Q

What are indicators?

A

Substances that change colour when they are added to acidic or basic solutions e.g. Litmus Paper

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24
Q

What colour is Litmus Paper in acids?

A

Red

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25
Q

What colour is Litmus Paper in bases?

A

Blue

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26
Q

What colour is Litmus Paper in neutral?

A

Violet

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27
Q

What colour is Methyl Orange in acids?

28
Q

What colour is Methyl Orange in bases?

29
Q

What colour is Methyl Orange in neutral?

30
Q

What is the equation for the reaction between metals and acids?

A

Metal + Acid —> Salt + Hydrogen

31
Q

What does hydrochloric acid become when it reacts with a metal?

A

A Metal Chloride.

32
Q

What does sulfuric acid become when it reacts with a metal?

A

A Metal Sulfate.

33
Q

What does nitric acid become when it reacts with a metal?

A

A Metal Nitrate.

34
Q

What is the equation for the reaction between metal oxides and acids?

A

Acid + Metal Oxide —> Salt + Water

35
Q

What is the equation for the reaction between metal hydroxides (alkalis) and acids?

A

Acid + Metal Hydroxide —> Salt + Water

36
Q

What is the equation for the reaction between metal carbonates and acids?

A

Acid + Metal Carbonate —> Salt + Water + Carbon Dioxide

37
Q

What is a neutralisation reaction?

A

When an acid and alkali react, yielding a salt and water.

38
Q

What is the equation for the heated reaction between ammonium salts and bases?

A

Base + Ammonium Salt —> Salt + Ammonia + Water

39
Q

What compound creates a colour change when it reacts?

A

Copper Sulfate

40
Q

Separating Mixtures Practical - Step 1

A

Use a Bunsen burner to gently warm the acid.

41
Q

Separating Mixtures Practical - Step 2

A

Add the insoluble solid (with stirring) until the reaction no longer happens.

42
Q

Separating Mixtures Practical - Step 3

A

Filter the solution to remove the excess insoluble solid and leave a solution of the salt dissolved in water.

43
Q

Separating Mixtures Practical - Step 4

A

Heat the solution in an evaporating basin above a beaker of water. The ‘water bath’ ensures gentle heating.

44
Q

Separating Mixtures Practical - Step 5

A

Let the solution cool and allow more water to evaporate. As water evaporates, the solution will become more concentrated and the salt will begin to crystallise.

45
Q

What is universal indicator?

A

The indicator changes to a particular colour depending on the pH of a solution.

46
Q

What is a pH probe?

A

The probe returns a number that represents the pH of a solution.

47
Q

Specifically, what is the pH scale a measure of?

A

The numerical pH scale is a measure of the concentration of H+ ions in a solution. For every increase of 1 in pH, the concentration of H+ ions gets divided by 10.

48
Q

What is the ionic equation for a neutralisation reaction?

A

H+(aq) + OH-(aq) —> H2O(l)

49
Q

What is titration?

A

Titration is a technique that measures the volumes of acid and base solutions that are needed in a neutralisation reaction.

50
Q

What are the variables of titration?

A

The concentration of the acid to be added and the volume of the base.

51
Q

What colour is Phenolphthalein in acids?

A

Colourless

52
Q

What colour is Phenolphthalein in bases?

53
Q

Which point of neutralisation reactions do titration indicators help us see?

54
Q

In titration calculations, what unit is concentration measured in?

55
Q

In titration calculations, what unit is volume measured in?

56
Q

What is the equation to find concentration?

A

Number of moles/Volume

57
Q

What is the equation to find the number of moles?

A

Concentration x Volume

58
Q

What is the equation to find volume?

A

Number of moles/Concentration

59
Q

1 dm3 is equal to how many cm3?

60
Q

Titration Calculations - Step 1

A

Write down the balanced symbol equation of the equation. Work out the ratio of reactants.

61
Q

Titration Calculations - Step 2

A

Divide the volume by 1000 if it’s in cm3. Then, work out how many moles of the known substance you have using the formula n=cV.

62
Q

Titration Calculations - Step 3

A

The number of moles for either substance follows the ratio found in Step 1. Complete any calculations necessary.

63
Q

Titration Calculations - Step 4

A

Work out the concentration/volume of the “unknown” substance using the equation c=n/V or V=n/c .

64
Q

What can be seen when a metal carbonate and an acid react?

A

Effervescence

65
Q

Which compound is used to test for sulfates?

A

Barium Chloride

66
Q

How can you test for sulfates?

A

Add Barium Chloride. If a white precipitate of Barium Sulfate is seen then a displacement reaction has happened.

67
Q

How do you separate a sulfate test?

A

Filter through filter paper, wash with distilled water and dry.

GCSE WJEC Chemistry (9 decks)

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