IGCSE Chemistry notes --> ACID BASES AND SALTS

1. ACIDS, BASESACIDS, BASES
& SALTS& SALTS
A guide for GCSE studentsA guide for GCSE students
KNOCKHARDY PUBLISHINGKNOCKHARDY PUBLISHING
20102010
SPECIFICATIONSSPECIFICATIONS

2. ACIDS, BASES & SALTSACIDS, BASES & SALTS
INTRODUCTION
This Powerpoint show is one of several produced to help students
understand selected GCSE Chemistry topics. It is based on the requirements
of the AQA specification but is suitable for other examination boards.
Individual students may use the material at home for revision purposes and
it can also prove useful for classroom teaching with an interactive white
board.
Accompanying notes on this, and the full range of AS and A2 Chemistry
topics, are available from the KNOCKHARDY WEBSITE at...
www.knockhardy.org.uk
All diagrams and animations in this Powerpoint are original and
created by Jonathan Hopton. Permission must be obtained for their
use in any commercial work.
All diagrams and animations in this Powerpoint are original and
created by Jonathan Hopton. Permission must be obtained for their
use in any commercial work.

3. CONTENTSCONTENTS
• Acidity and alkalinity
• Indicators
• pH
• Acids
• General methods for making salts
• Making salts from metal oxides
• Making salts from metal carbonates
• Making salts from metals
• Making salts from alkalis – by titration
• Making insoluble salts – by precipitation
• Questions
ACIDS, BASES & SALTSACIDS, BASES & SALTS

4. ACIDITY AND ALKALINITYACIDITY AND ALKALINITY
• water is a neutral substance
• when substances dissolve in water, the solution may become…
ACIDIC or ALKALINE or stay NEUTRAL

5. ACIDITY AND ALKALINITYACIDITY AND ALKALINITY
• water is a neutral substance
• when substances dissolve in water, the solution may become…
ACIDIC or ALKALINE or stay NEUTRAL
• hydrogen ions H+
(aq) make solutions acidic
• hydroxide ions OH¯(aq) make solutions alkaline
• solutions with equal numbers of H+
(aq) and OH¯(aq) are neutral

6. INDICATORSINDICATORS
• show by a colour change if a solution is acidic, alkaline or neutral
• some can even show how acidic or how alkaline a solution is

7. INDICATORSINDICATORS
• show by a colour change if a solution is acidic, alkaline or neutral
• some can even show how acidic or how alkaline a solution is
• well known indicators include…

8. INDICATORSINDICATORS
• show by a colour change if a solution is acidic, alkaline or neutral
• some can even show how acidic or how alkaline a solution is
• well known indicators include…
LITMUS
acidic RED alkaline BLUE neutral PURPLE

9. INDICATORSINDICATORS
• show by a colour change if a solution is acidic, alkaline or neutral
• some can even show how acidic or how alkaline a solution is
• well known indicators include…
LITMUS
acidic RED alkaline BLUE neutral PURPLE

10. INDICATORSINDICATORS
• show by a colour change if a solution is acidic, alkaline or neutral
• some can even show how acidic or how alkaline a solution is
• well known indicators include…
LITMUS
acidic RED alkaline BLUE neutral PURPLE
UNIVERSAL
acidic RED alkaline VIOLET neutral GREEN

11. INDICATORSINDICATORS
• show by a colour change if a solution is acidic, alkaline or neutral
• some can even show how acidic or how alkaline a solution is
• well known indicators include…
LITMUS
acidic RED alkaline BLUE neutral PURPLE
UNIVERSAL
acidic RED alkaline VIOLET neutral GREEN

12. pH SCALEpH SCALE

13. pH SCALEpH SCALE
Used to compare the relative acidity (and alkalinity) of solutions.
The value is related to the concentration of H+
ions, in solution.

14. pH SCALEpH SCALE
Used to compare the relative acidity (and alkalinity) of solutions.
The value is related to the concentration of H+
ions, in solution.
“The greater the concentration of hydrogen ions
in solution, the lower the pH”

15. pH SCALEpH SCALE
Used to compare the relative acidity (and alkalinity) of solutions.
The value is related to the concentration of H+
ions, in solution.
“The greater the concentration of hydrogen ions
in solution, the lower the pH”
<— 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 —>
strongly weakly neutral weakly strongly
acidic acidic alkaline alkaline

16. pH SCALEpH SCALE
Used to compare the relative acidity (and alkalinity) of solutions.
The value is related to the concentration of H+
ions, in solution.
“The greater the concentration of hydrogen ions
in solution, the lower the pH”
<— 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 —>
strongly weakly neutral weakly strongly
acidic acidic alkaline alkaline
HCl CH3COOH H2O NH3 NaOH
HYDROCHLORIC ETHANOIC AMMONIA SODIUM
ACID ACID HYDROXIDE

17. pH SCALEpH SCALE
Used to compare the relative acidity (and alkalinity) of solutions.
The value is related to the concentration of H+
ions, in solution.
“The greater the concentration of hydrogen ions
in solution, the lower the pH”
<— 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 —>
strongly weakly neutral weakly strongly
acidic acidic alkaline alkaline
HCl CH3COOH H2O NH3 NaOH
HYDROCHLORIC ETHANOIC AMMONIA SODIUM
ACID ACID HYDROXIDE
Acidic solutions pH < 7
Alkaline solutions pH > 7
Neutral solutions pH = 7

18. pH SCALEpH SCALE
Despite what some people think, the pH scale is not restricted to
between 0 and 14. It extends beyond those values, but is not as
relevant; e.g. the pH of the dilute HCl and H2SO4 found on the
laboratory shelves is -0.3 and -0.6 respectively.

19. pH SCALEpH SCALE
Despite what some people think, the pH scale is not restricted to
between 0 and 14. It extends beyond those values, but is not as
relevant; e.g. the pH of the dilute HCl and H2SO4 found on the
laboratory shelves is -0.3 and -0.6 respectively.
Weak acids have higher pH values than stronger ones of the same
concentration.
Ethanoic acid CH3COOH has a larger pH than
hydrochloric acid HCl of the same concentration.

20. MEASURING pHMEASURING pH
Indicator Add a few drops of universal (full-range) indicator to
the solution and compare the colour against a chart.
The colour you “see” depends not only on how many
drops of indicator you add but also on your perception
of colour.

21. MEASURING pHMEASURING pH
Indicator Add a few drops of universal (full-range) indicator to
the solution and compare the colour against a chart.
The colour you “see” depends not only on how many
drops of indicator you add but also on your perception
of colour.
pH meters Electrical/electronic devices which measure the
conductivity of the solution.
Having calibrated the apparatus against a solution of
known pH, you place the probe in any solution and read
off the pH value on a scale or digital read-out.

22. ACIDSACIDS

23. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can be arranged into groups according to
how many H+
ions they produce from each molecule

24. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can be arranged into groups according to
how many H+
ions they produce from each molecule
ACID SALTS ION EXAMPLE
hydrochloric HCl chloride Cl¯ NaCl
nitric HNO3 nitrate NO3¯ NaNO3
ethanoic CH3COOH ethanoate CH3COO¯ CH3COONa
THE ABOVE ARE MONOPROTIC (MONOBASIC) ACIDS

25. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can be arranged into groups according to
how many H+
ions they produce from each molecule
ACID SALTS ION EXAMPLE
hydrochloric HCl chloride Cl¯ NaCl
nitric HNO3 nitrate NO3¯ NaNO3
ethanoic CH3COOH ethanoate CH3COO¯ CH3COONa
THE ABOVE ARE MONOPROTIC (MONOBASIC)ACIDS
sulphuric H2SO4 hydrogensulphate HSO4¯ NaHSO4
sulphate SO4
2-
Na2SO4
“carbonic” H2CO3 hydrogencarbonate HCO3¯ NaHCO3
carbonate CO3
2-
Na2CO3

26. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can also arranged into groups according to
the extent they split into ions when put in water.

27. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can also arranged into groups according to
the extent they split into ions when put in water.
STRONG ACIDS COMPLETELY dissociate (split up) into ions
e.g. sulphuric, hydrochloric, nitric

28. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can also arranged into groups according to
the extent they split into ions when put in water.
STRONG ACIDS COMPLETELY dissociate (split up) into ions
e.g. sulphuric, hydrochloric, nitric
WEAK ACIDS PARTIALLY dissociate (split up) into ions
e.g. ethanoic, citric, carbonic

29. ACIDSACIDS
Definition ACIDS ARE PROTON (H+
ion) DONORS
Categories Acids can also arranged into groups according to
the extent they split into ions when put in water.
STRONG ACIDS COMPLETELY dissociate (split up) into ions
e.g. sulphuric, hydrochloric, nitric
WEAK ACIDS PARTIALLY dissociate (split up) into ions
e.g. ethanoic, citric, carbonic
This means that if you take similar concentrations of HCl and
CH3COOH, the concentration of H+
ions in the solution of CH3COOH
will be less as only a few of its molecules will have split up into ions.
Its pH will consequently be higher.

30. ACIDSACIDS
Reactions The hydrogen ions produced by acids can be replaced
by other positive ions (metal ions or ammonium ions)
to produce salts. This occurs when dilute acids react
with metals, oxides of metals, hydroxides of metals,
carbonates, hydrogencarbonates and ammonia.

31. ACIDSACIDS
Reactions The hydrogen ions produced by acids can be replaced
by other positive ions (metal ions or ammonium ions)
to produce salts. This occurs when dilute acids react
with metals, oxides of metals, hydroxides of metals,
carbonates, hydrogen carbonates and ammonia.
HYDROCHLORIC ACID
ZINC
CHLORIDE
SODIUM
CHLORIDE
COPPER
CHLORIDE
AMMONIUM
CHLORIDEZINC
SODIUM HYDROXIDE
COPPER OXIDE
AMMONIA
MAGNESIUM
CHLORIDE
MAGNESIUM
CARBONATE

32. ACIDSACIDS
Reactions The hydrogen ions produced by acids can be replaced
by other positive ions (metal ions or ammonium ions)
to produce salts. This occurs when dilute acids react
with metals, oxides of metals, hydroxides of metals,
carbonates, hydrogen carbonates and ammonia.
SULPHURIC ACID
ZINC
SULPHATE
SODIUM
SULPHATE
COPPER
SULPHATE
AMMONIUM
SULPHATEZINC
SODIUM HYDROXIDE
COPPER OXIDE
AMMONIA
MAGNESIUM
SULPHATE
MAGNESIUM
CARBONATE

33. MAKING SALTS - POSSIBILITIESMAKING SALTS - POSSIBILITIES
IS THE SALT SOLUBLE
OR INSOLUBLE?
DOES THE METAL
REACT WITH DILUTE
ACIDS?
IS IT
SAFE?
IS THE METAL OXIDE
OR CARBONATE
SOLUBLE IN WATER?
MIX SOLUTIONS OF
TWO SUITABLE
SALTS TO
PRECIPITATE THE
INSOLUBLE SALT
ADD EXCESS METAL
TO THE ACID THEN
FILTER OFF THE
EXCESS METAL
TITRATE THE METAL
HYDROXIDE WITH
ACID
FILTER OFF
THE SALT
ADD EXCESS METAL
OXIDE OR METAL
CARBONATE TO ACID
THEN FILTER OFF THE
EXCESS SOLID
CRYSTALLISE
THE SALT
FROM THE
FILTRATE
NONO
SOLUBLE
NO
YES
YESYES
INSOLUBLE

34. PREPARATION OF SOLUBLE SALTSPREPARATION OF SOLUBLE SALTS
Salts can be made by NEUTRALISATION of acids;
• acidic solutions contain aqueous hydrogen ions H+
(aq)
• sulphuric acid produces a sulphate
• hydrochloric acid produces a chloride
• nitric acid produces a nitrate

35. Salts can be made by NEUTRALISATION of acids;
• acidic solutions contain aqueous hydrogen ions H+
(aq)
• sulphuric acid produces a sulphate
• hydrochloric acid produces a chloride
• nitric acid produces a nitrate
Other chemicals are formed, it depends on what is neutralising the acid.
OXIDES SALT + WATER
HYDROXIDES SALT + WATER
CARBONATES SALT + CARBON DIOXIDE + WATER
METALS SALT + HYDROGEN
(not all metals are suitable; some are too reactive; others are not reactive enough)
PREPARATION OF SOLUBLE SALTSPREPARATION OF SOLUBLE SALTS

36. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

37. MAKING SALTS – FROM INSOLUBLE BASESMAKING SALTS – FROM INSOLUBLE BASES
IS THE SALT SOLUBLE
OR INSOLUBLE?
DOES THE METAL
REACT WITH DILUTE
ACIDS?
IS IT
SAFE?
IS THE METAL OXIDE
OR CARBONATE
SOLUBLE IN WATER?
MIX SOLUTIONS OF
TWO SUITABLE
SALTS TO
PRECIPITATE THE
INSOLUBLE SALT
ADD EXCESS METAL
TO THE ACID THEN
FILTER OFF THE
EXCESS METAL
TITRATE THE METAL
HYDROXIDE WITH
ACID
FILTER OFF
THE SALT
ADD EXCESS METAL
OXIDE OR METAL
CARBONATE TO ACID
THEN FILTER OFF THE
EXCESS SOLID
CRYSTALLISE
THE SALT
FROM THE
FILTRATE
NONO
SOLUBLE
NO
YES
YESYES
INSOLUBLE

38. Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

39. 1 Place dilute acid in a beaker and warm it
gently without letting it boil (reactions are
faster at higher temperatures)
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

40. 1 Place dilute acid in a beaker and warm it
gently without letting it boil (reactions are
faster at higher temperatures)
2. Remove the heat
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

41. 1 Place dilute acid in a beaker and warm it
gently without letting it boil (reactions are
faster at higher temperatures)
2. Remove the heat
3. Carefully and slowly add small amounts of
the solid while stirring (most reactions of
this type are exothermic i.e. they give off
energy - the energy released would make
the solution boil over)
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

42. 1 Place dilute acid in a beaker and warm it
gently without letting it boil (reactions are
faster at higher temperatures)
2. Remove the heat
3. Carefully and slowly add small amounts of
the solid while stirring (most reactions of
this type are exothermic i.e. they give off
energy - the energy released would make
the solution boil over)
4. Continue adding the solid until no more
dissolves (this ensures all the acid has
been used - it is easier to filter off excess
solid than extract excess acid).
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

43. 5. Filter the solution into an evaporating dish
to remove excess solid
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

44. 5. Filter the solution into an evaporating dish
to remove excess solid
6. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

45. 5. Filter the solution into an evaporating dish
to remove excess solid
6. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
7. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess insoluble oxideAcid with excess insoluble oxide
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

46. 5. Filter the solution into an evaporating dish
to remove excess solid
6. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
7. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess insoluble oxideAcid with excess insoluble oxide
8. When sufficient crystals have appeared, filter them off, wash with a little
cold water and transfer them to a filter paper. Place another filter paper
over the top and press gently to help remove some of the water.
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

47. 5. Filter the solution into an evaporating dish
to remove excess solid
6. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
7. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess insoluble oxideAcid with excess insoluble oxide
8. When sufficient crystals have appeared, filter them off, wash with a little
cold water and transfer them to a filter paper. Place another filter paper
over the top and press gently to help remove some of the water.
9. Allow the crystals to dry naturally in air. (heat can cause the crystals to
decompose and lose their water of crystallisation)
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

48. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess insoluble carbonateAcid with excess insoluble carbonate

49. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
The method used is similar to that used with acids and metal oxides.
The main differences is that it is not necessary to use heat and that
carbon dioxide gas is given off so you have to make sure the solution
doesn’t effervesce (fizz) too much.

50. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
The method used is similar to that used with acids and metal oxides.
The main differences is that it is not necessary to use heat and that
carbon dioxide gas is given off so you have to make sure the solution
doesn’t effervesce (fizz) too much.
1 Place dilute acid in a beaker

51. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
The method used is similar to that used with acids and metal oxides.
The main differences is that it is not necessary to use heat and that
carbon dioxide gas is given off so you have to make sure the solution
doesn’t effervesce (fizz) too much.
1 Place dilute acid in a beaker
2. Carefully and slowly add small amounts of
the solid carbonate while stirring – make
sure there is not too much effervescence.

52. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
The method used is similar to that used with acids and metal oxides.
The main differences is that it is not necessary to use heat and that
carbon dioxide gas is given off so you have to make sure the solution
doesn’t effervesce (fizz) too much.
1 Place dilute acid in a beaker
2. Carefully and slowly add small amounts of
the solid carbonate while stirring – make
sure there is not too much effervescence.
3. Continue adding the solid carbonate until
no more dissolves (this ensures all the
acid has been used - it is easier to filter off
excess solid than extract excess acid).

53. 4. Filter the solution into an evaporating dish
to remove excess solid
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

54. 4. Filter the solution into an evaporating dish
to remove excess solid
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

55. 4. Filter the solution into an evaporating dish
to remove excess solid
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
6. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

56. 4. Filter the solution into an evaporating dish
to remove excess solid
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
6. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
7. When sufficient crystals have appeared, filter them off, wash with a little
cold water and transfer them to a filter paper. Place another filter paper
over the top and press gently to help remove some of the water.
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

57. 4. Filter the solution into an evaporating dish
to remove excess solid
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
6. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess insoluble carbonateAcid with excess insoluble carbonate
7. When sufficient crystals have appeared, filter them off, wash with a little
cold water and transfer them to a filter paper. Place another filter paper
over the top and press gently to help remove some of the water.
8. Allow the crystals to dry naturally in air. (heat can cause the crystals to
decompose and lose their water of crystallisation)
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

58. MAKING SALTS – FROM METALSMAKING SALTS – FROM METALS
IS THE SALT SOLUBLE
OR INSOLUBLE?
DOES THE METAL
REACT WITH DILUTE
ACIDS?
IS IT
SAFE?
IS THE METAL OXIDE
OR CARBONATE
SOLUBLE IN WATER?
MIX SOLUTIONS OF
TWO SUITABLE
SALTS TO
PRECIPITATE THE
INSOLUBLE SALT
ADD EXCESS METAL
TO THE ACID THEN
FILTER OFF THE
EXCESS METAL
TITRATE THE METAL
HYDROXIDE WITH
ACID
FILTER OFF
THE SALT
ADD EXCESS METAL
OXIDE OR METAL
CARBONATE TO ACID
THEN FILTER OFF THE
EXCESS SOLID
CRYSTALLISE
THE SALT
FROM THE
FILTRATE
NONO
SOLUBLE
NO
YES
YESYES
INSOLUBLE

59. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess metalAcid with excess metal

60. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess metalAcid with excess metal
The method used is similar to that used with acids and metal oxides
or metal carbonates. However, because hydrogen is produced during
the experiment, Bunsen burners must not be used while the chemical
reaction is taking place.
Not all metals are suitable: some are too reactive K, Na, Ca
some don’t react Cu

61. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess metalAcid with excess metal
The method used is similar to that used with acids and metal oxides
or metal carbonates. However, because hydrogen is produced during
the experiment, Bunsen burners must not be used while the chemical
reaction is taking place.
Not all metals are suitable: some are too reactive K, Na, Ca
some don’t react Cu
1 Place dilute acid in a beaker

62. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess metalAcid with excess metal
The method used is similar to that used with acids and metal oxides
or metal carbonates. However, because hydrogen is produced during
the experiment, Bunsen burners must not be used while the chemical
reaction is taking place.
Not all metals are suitable: some are too reactive K, Na, Ca
some don’t react Cu
1 Place dilute acid in a beaker
2. Carefully and slowly add small amounts of
the metal while stirring – make sure there
is not too much effervescence.

63. PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION
Acid with excess metalAcid with excess metal
The method used is similar to that used with acids and metal oxides
or metal carbonates. However, because hydrogen is produced during
the experiment, Bunsen burners must not be used while the chemical
reaction is taking place.
Not all metals are suitable: some are too reactive K, Na, Ca
some don’t react Cu
1 Place dilute acid in a beaker
2. Carefully and slowly add small amounts of
the metal while stirring – make sure there
is not too much effervescence.
3. Continue adding the metal until no more
dissolves (this ensures all the acid has
been used - it is easier to filter off excess
metal than extract excess acid).

64. 4. Filter the solution into an evaporating dish
to remove excess metal
Acid with excess metalAcid with excess metal
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

65. 4. Filter the solution into an evaporating dish
to remove excess metal
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
Acid with excess metalAcid with excess metal
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

66. 4. Filter the solution into an evaporating dish
to remove excess metal
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
6. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess metalAcid with excess metal
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

67. 4. Filter the solution into an evaporating dish
to remove excess metal
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
6. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess metalAcid with excess metal
7. When sufficient crystals have appeared, filter them off, wash with a little
cold water and transfer them to a filter paper. Place another filter paper
over the top and press gently to help remove some of the water.
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

68. 4. Filter the solution into an evaporating dish
to remove excess metal
5. Transfer the dish to a tripod and carefully
warm the mixture to remove some of the
water. Too much heat will drive off any
water of crystallisation.
6. When some of the water has been
evaporated, let the solution to cool;
(allows crystallisation takes place)
Acid with excess metalAcid with excess metal
7. When sufficient crystals have appeared, filter them off, wash with a little
cold water and transfer them to a filter paper. Place another filter paper
over the top and press gently to help remove some of the water.
8. Allow the crystals to dry naturally in air. (heat can cause the crystals to
decompose and lose their water of crystallisation)
PREPARATION OF SALTS BY NEUTRALISATIONPREPARATION OF SALTS BY NEUTRALISATION

69. MAKING SALTS – FROM SOLUBLE BASES (ALKALIS)MAKING SALTS – FROM SOLUBLE BASES (ALKALIS)
IS THE SALT SOLUBLE
OR INSOLUBLE?
DOES THE METAL
REACT WITH DILUTE
ACIDS?
IS IT
SAFE?
IS THE METAL OXIDE
OR CARBONATE
SOLUBLE IN WATER?
MIX SOLUTIONS OF
TWO SUITABLE
SALTS TO
PRECIPITATE THE
INSOLUBLE SALT
ADD EXCESS METAL
TO THE ACID THEN
FILTER OFF THE
EXCESS METAL
TITRATE THE METAL
HYDROXIDE WITH
ACID
FILTER OFF
THE SALT
ADD EXCESS METAL
OXIDE OR METAL
CARBONATE TO ACID
THEN FILTER OFF THE
EXCESS SOLID
CRYSTALLISE
THE SALT
FROM THE
FILTRATE
NONO
SOLUBLE
NO
YES
YESYES
INSOLUBLE

70. ALKALISALKALIS

71. ALKALISALKALIS
Definition ALKALIS ARE SOLUBLE BASES
Their solutions contain hydroxide ions, OH¯(aq)

72. ALKALISALKALIS
Definition ALKALIS ARE SOLUBLE BASES
Their solutions contain hydroxide ions, OH¯(aq)
STRONG ALKALIS sodium hydroxide (NaOH)
potassium hydroxide (KOH)
WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)

73. ALKALISALKALIS
Definition ALKALIS ARE SOLUBLE BASES
Their solutions contain hydroxide ions, OH¯(aq)
STRONG ALKALIS sodium hydroxide (NaOH)
potassium hydroxide (KOH)
WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)
Making salts using alkalis cannot be done by the methods used for
insoluble bases because you cannot tell when all the acid has been
neutralised – the excess alkali is soluble.

74. ALKALISALKALIS
Definition ALKALIS ARE SOLUBLE BASES
Their solutions contain hydroxide ions, OH¯(aq)
STRONG ALKALIS sodium hydroxide (NaOH)
potassium hydroxide (KOH)
WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)
Making salts using alkalis cannot be done by the methods used for
insoluble bases because you cannot tell when all the acid has been
neutralised – the excess alkali is soluble.
The salts are made by titration using an indicator
ACID + ALKALINE HYDROXIDE ——> NEUTRAL SALT + WATER
SOLUTION SOLUTION

75. ALKALISALKALIS
Definition ALKALIS ARE SOLUBLE BASES
Their solutions contain hydroxide ions, OH¯(aq)
STRONG ALKALIS sodium hydroxide (NaOH)
potassium hydroxide (KOH)
WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)
Making salts using alkalis cannot be done by the methods used for
insoluble bases because you cannot tell when all the acid has been
neutralised – the excess alkali is soluble.
The salts are made by titration using an indicator
ACID + ALKALINE HYDROXIDE ——> NEUTRAL SALT + WATER
SOLUTION SOLUTION
The indicator tells you when the acid has been neutralised

76. AMMONIUM SALTSAMMONIUM SALTS
Ammonia is very soluble in water giving an alkaline solution which
can be neutralised by acids to produce AMMONIUM SALTS
e.g. AMMONIA + HYDROCHLORIC —> AMMONIUM
SOLUTION ACID CHLORIDE

77. AMMONIUM SALTSAMMONIUM SALTS
Ammonia is very soluble in water giving an alkaline solution which
can be neutralised by acids to produce AMMONIUM SALTS
e.g. AMMONIA + HYDROCHLORIC —> AMMONIUM
SOLUTION ACID CHLORIDE
If ammonium hydroxide is specified you can write the equation
AMMONIUM + HYDROCHLORIC —> AMMONIUM + WATER
HYDROXIDE ACID CHLORIDE
Ammonium salts make very important fertilisers

78. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3

79. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.

80. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

81. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

82. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

83. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

84. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

85. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

86. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
This method is limited to the soluble salts of ammonia or alkali metals
e.g. ammonium chloride NH4Cl
sodium chloride NaCl
potassium sulphate K2SO4
sodium nitrate NaNO3
Method React an acid with an alkali (hydroxides of Group I
metals and ammonia). The method involves TITRATION.
1 Place a measured quantity of acid in a conical flask.
2 Add three or four drops of a suitable indicator.
3 Place the alkali in a burette. Note the level of the liquid.
4 Add the alkali to the acid until the indicator just changes colour
Note the new level of liquid.
5 Repeat experiment with exactly the same volumes but no indicator.
6 Evaporate a small amount of the water in an evaporating basin and
let the solution cool to allow crystals to form.

87. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
Example word equations:-
sodium hydroxide + hydrochloric acid —> sodium chloride + water
sodium hydroxide + sulphuric acid —> sodium sulphate + water
potassium hydroxide + nitric acid —> potassium nitrate + water
ammonium hydroxide + nitric acid —> ammonium nitrate + water

88. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
Example word equations:-
sodium hydroxide + hydrochloric acid —> sodium chloride + water
sodium hydroxide + sulphuric acid —> sodium sulphate + water
potassium hydroxide + nitric acid —> potassium nitrate + water
ammonium hydroxide + nitric acid —> ammonium nitrate + water
Now complete these:-

89. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
Example word equations:-
sodium hydroxide + hydrochloric acid —> sodium chloride + water
sodium hydroxide + sulphuric acid —> sodium sulphate + water
potassium hydroxide + nitric acid —> potassium nitrate + water
ammonium hydroxide + nitric acid —> ammonium nitrate + water
Now complete these:-
potassium hydroxide + hydrochloric acid —> potassium chloride + water

90. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
Example word equations:-
sodium hydroxide + hydrochloric acid —> sodium chloride + water
sodium hydroxide + sulphuric acid —> sodium sulphate + water
potassium hydroxide + nitric acid —> potassium nitrate + water
ammonium hydroxide + nitric acid —> ammonium nitrate + water
Now complete these:-
potassium hydroxide + hydrochloric acid —> potassium chloride + water
sodium hydroxide + nitric acid —> sodium nitrate + water

91. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
Example word equations:-
sodium hydroxide + hydrochloric acid —> sodium chloride + water
sodium hydroxide + sulphuric acid —> sodium sulphate + water
potassium hydroxide + nitric acid —> potassium nitrate + water
ammonium hydroxide + nitric acid —> ammonium nitrate + water
Now complete these:-
potassium hydroxide + hydrochloric acid —> potassium chloride + water
sodium hydroxide + nitric acid —> sodium nitrate + water
ammonium hydroxide + hydrochloric acid —> ammonium chloride + water

92. MAKING SALTS BY TITRATIONMAKING SALTS BY TITRATION
Example word equations:-
sodium hydroxide + hydrochloric acid —> sodium chloride + water
sodium hydroxide + sulphuric acid —> sodium sulphate + water
potassium hydroxide + nitric acid —> potassium nitrate + water
ammonium hydroxide + nitric acid —> ammonium nitrate + water
Now complete these:-
potassium hydroxide + hydrochloric acid —> potassium chloride + water
sodium hydroxide + nitric acid —> sodium nitrate + water
ammonium hydroxide + hydrochloric acid —> ammonium chloride + water

93. NEUTRALISATION - IONIC EQUATIONNEUTRALISATION - IONIC EQUATION
In all alkali – acid reactions, the same ionic reaction takes place…

94. NEUTRALISATION - IONIC EQUATIONNEUTRALISATION - IONIC EQUATION
In all alkali – acid reactions, the same ionic reaction takes place…
sodium hydroxide + dil. nitric acid —> sodium nitrate + water
NaOH(aq) + HNO3 (aq) —> NaNO3 (aq) + H2O (l)

95. NEUTRALISATION - IONIC EQUATIONNEUTRALISATION - IONIC EQUATION
In all alkali – acid reactions, the same ionic reaction takes place…
sodium hydroxide + dil. nitric acid —> sodium nitrate + water
NaOH(aq) + HNO3 (aq) —> NaNO3 (aq) + H2O (l)
Na+
(aq) + OH¯(aq) + H+
(aq) + NO3¯(aq) —> Na+
(aq) + NO3¯(aq) + H2O(l)

96. NEUTRALISATION - IONIC EQUATIONNEUTRALISATION - IONIC EQUATION
In all alkali – acid reactions, the same ionic reaction takes place…
sodium hydroxide + dil. nitric acid —> sodium nitrate + water
NaOH(aq) + HNO3 (aq) —> NaNO3 (aq) + H2O (l)
Na+
(aq) + OH¯(aq) + H+
(aq) + NO3¯(aq) —> Na+
(aq) + NO3¯(aq) + H2O(l)
cancel ions H+
(aq) + OH¯(aq) —> H2O(l)
from from
acid alkali

97. MAKING SALTS - POSSIBILITIESMAKING SALTS - POSSIBILITIES
IS THE SALT SOLUBLE
OR INSOLUBLE?
DOES THE METAL
REACT WITH DILUTE
ACIDS?
IS IT
SAFE?
IS THE METAL OXIDE
OR CARBONATE
SOLUBLE IN WATER?
MIX SOLUTIONS OF
TWO SUITABLE
SALTS TO
PRECIPITATE THE
INSOLUBLE SALT
ADD EXCESS METAL
TO THE ACID THEN
FILTER OFF THE
EXCESS METAL
TITRATE THE METAL
HYDROXIDE WITH
ACID
FILTER OFF
THE SALT
ADD EXCESS METAL
OXIDE OR METAL
CARBONATE TO ACID
THEN FILTER OFF THE
EXCESS SOLID
CRYSTALLISE
THE SALT
FROM THE
FILTRATE
NONO
SOLUBLE
NO
YES
YESYES
INSOLUBLE

98. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS

99. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.

100. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
EXAMPLES silver chloride silver nitrate and sodium chloride
barium sulphate barium chloride and sodium sulphate
lead iodide lead nitrate and potassium iodide

101. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.

102. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
Prepare a solution of sodium chloride.1

103. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
The sodium chloride lattice breaks up and dissolves in the water.2

104. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
Prepare a solution of silver nitrate.3

105. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
The silver nitrate lattice breaks up and dissolves in the water.4

106. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
Mix the two solutions.5

107. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
All four ions are now mixed together.6

108. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
The silver ions and chloride ions come together and the
insoluble silver chloride forms a white precipitate.
7

109. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.
Because sodium nitrate is soluble in water their ions remain in
solution. The precipitate is then filtered, washed and dried.
7

110. PREPARATION OF INSOLUBLE SALTSPREPARATION OF INSOLUBLE SALTS
METHOD Insoluble salts can be made by mixing appropriate
solutions of ions so that a precipitate is formed.
PREPARATION OF SILVER CHLORIDE
To make silver chloride you need…
(i) a soluble silver salt silver nitrate plus
(ii) a soluble chloride sodium chloride.

111. SALTS - QUESTIONSSALTS - QUESTIONS

112. SALTS - QUESTIONSSALTS - QUESTIONS
1. Work out what you get if the following chemicals are mixed.
a) zinc and sulphuric acid
b) copper carbonate and nitric acid
c) sodium hydroxide and hydrochloric acid
d) lead oxide and nitric acid
e) magnesium and hydrochloric acid
f) ammonium hydroxide and sulphuric acid
g) magnesium carbonate and sulphuric acid

113. SALTS - QUESTIONSSALTS - QUESTIONS
1. Work out what you get if the following chemicals are mixed.
a) zinc and sulphuric acid zinc sulphate + hydrogen
b) copper carbonate and nitric acid copper nitrate + carbon dioxide + water
c) sodium hydroxide and hydrochloric acid sodium chloride + water
d) lead oxide and nitric acid lead nitrate + water
e) magnesium and hydrochloric acid magnesium chloride + hydrogen
f) ammonium hydroxide and sulphuric acid ammonium sulphate + water
g) magnesium carbonate and sulphuric acid magnesium + carbon + water
sulphate dioxide

114. SALTS - QUESTIONSSALTS - QUESTIONS
1. Work out what you get if the following chemicals are mixed.
a) zinc and sulphuric acid zinc sulphate + hydrogen
b) copper carbonate and nitric acid copper nitrate + carbon dioxide + water
c) sodium hydroxide and hydrochloric acid sodium chloride + water
d) lead oxide and nitric acid lead nitrate + water
e) magnesium and hydrochloric acid magnesium chloride + hydrogen
f) ammonium hydroxide and sulphuric acid ammonium sulphate + water
g) magnesium carbonate and sulphuric acid magnesium + carbon + water
sulphate dioxide
2. Answer the following...
Which ion is found in (i) acidic solutions; H+
(aq) (ii) alkaline solutions?
What is formed when you mix these two ions together?
What name do we give to this type of reaction?
When making salts from metals, oxides and carbonates, how do you know
when all the acid is used up?
When making salts from soluble Group I hydroxides, what do
you use to check when all the acid is used up?

115. SALTS - QUESTIONSSALTS - QUESTIONS
1. Work out what you get if the following chemicals are mixed.
a) zinc and sulphuric acid zinc sulphate + hydrogen
b) copper carbonate and nitric acid copper nitrate + carbon dioxide + water
c) sodium hydroxide and hydrochloric acid sodium chloride + water
d) lead oxide and nitric acid lead nitrate + water
e) magnesium and hydrochloric acid magnesium chloride + hydrogen
f) ammonium hydroxide and sulphuric acid ammonium sulphate + water
g) magnesium carbonate and sulphuric acid magnesium + carbon + water
sulphate dioxide
2. Answer the following...
Which ion is found in (i) acidic solutions; H+
(aq) (ii) alkaline solutions? OH¯(aq)
What is formed when you mix these two ions together? WATER
What name do we give to this type of reaction? NEUTRALISATION
When making salts from metals, oxides and carbonates, how do you know
when all the acid is used up? WHEN THE SOLID NO LONGER DISSOLVES
When making salts from soluble Group I hydroxides, what do
you use to check when all the acid is used up? AN INDICATOR

116. ACIDS, BASESACIDS, BASES
& SALTS& SALTS
THE ENDTHE END
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