
6c. MAKING an INSOLUBLE SALT BY A PRECIPITATION REACTION
Doc
Brown's Chemistry GCSE/IGCSE/O level Science–Chemistry Revision Notes
The pH scale of acidity and alkalinity,
acids, alkalis, salts and neutralisation
6. Methods of
making salts:
6c. How to make an insoluble salt by a
precipitation reaction
Sub-index
for this page
Introduction and solubilities of salts
The method
of making a salt by precipitation
The
preparation of silver chloride
The
preparation of lead(II) iodide
The
preparation of calcium carbonate
The
preparation of barium sulfate
The
preparation of lead(II) sulfate
The
preparation of calcium sulfate
The uses of some
insoluble salts
Method (a)
Making a salt by neutralising a soluble acid with a soluble base (alkali) –
neutralisation reaction
Method (b)
preparing a salt by reacting an acid with a metal or an
insoluble base – oxide, hydroxide or carbonate
Method (c) Preparing an
insoluble salt by mixing solutions of two soluble compounds (this page)
Method (d) Making a
salt by directly combining its constituent elements
GCSE/IGCSE Acids & Alkalis revision notes sub–index:
Index of all pH, Acids, Alkalis, Salts Notes 1.
Examples of everyday acids, alkalis, salts, pH of
solution, hazard warning signs : 2.
pH scale, indicators, ionic theory of acids–alkali neutralisation : 4.
Reactions of acids with
metals/oxides/hydroxides/carbonates, neutralisation reactions : 5.
Reactions of bases–alkalis
like ammonia & sodium hydroxide : 6. Four methods
of making salts : 7. Changes in pH in a
neutralisation, choice and use of indicators : 8. Important formulae
of compounds, salt solubility and water of crystallisation :
10.
More on Acid–Base Theory and Weak and Strong Acids
See also
Advanced Level Chemistry Students Acid–Base Revision
Notes – use index
Doc Brown's
chemistry revision notes: basic school chemistry science GCSE chemistry, IGCSE chemistry, O level
& ~US grades 8, 9, 10 school science courses for ~14-16 year old science
students for national examinations in chemistry topics including acids bases
alkalis salts preparations reactions
6. METHODS of MAKING SALTS – salt
preparation procedures
6c.
Method (c) Preparing an Insoluble Salt
by a precipitation reaction
The procedure involves making an insoluble
salt my mixing solutions of soluble compounds to form a precipitate.
The two
soluble compounds must each provide one of the constituent ions of the desired
insoluble salt which precipitates out when the solutions are mixed.
NOTE definition: A precipitation reaction is generally defined as 'the formation of an
insoluble solid on mixing two solutions of soluble substances or bubbling a gas into a solution'.
Note that several
precipitation reactions are used as
simple tests
for e.g. for sulfate, chloride, bromide, iodide
Salt solubility affects the method you
choose to make a salt, the table below will help you decide on the method
A solubility guide
for salts and other compounds
Information required to decide on the method used to
prepare a salt |
salts and other compounds |
solubility? |
common salts of sodium, potassium and
ammonium ions |
usually soluble in water |
common sulfates (sulfates) |
usually quite soluble except for
calcium sulfate (slightly soluble), lead sulfate and barium
sulfate are both insoluble |
common chlorides (similar rule for
bromides and iodides) |
usually soluble except for insoluble
lead(II) chloride and silver chloride |
common nitrates |
all soluble |
common carbonates |
most metal carbonates are insoluble
apart from sodium & potassium carbonate. Ammonium carbonate is
also soluble. |
common hydroxides |
most metal hydroxides are insoluble apart from
sodium, potassium and ammonium hydroxide |
General rules
which describe the solubility of common types of compounds in water:
-
All common sodium,
potassium and ammonium salts are soluble e.g. NaCl, K2SO4,
NH4NO3
-
All nitrate salts are
soluble e.g. NaNO3, Mg(NO3)2, Al(NO3)3,
NH4NO3
-
Some ethanoate salts are
soluble e.g. CH3COONa
-
Common chloride salts are
soluble except those of silver and lead e.g.
-
Common sulfates are
soluble except those of lead, barium and calcium: soluble e.g.
-
soluble: Na2SO4,
MgSO4, Al2(SO4)3
-
insoluble: PbSO4,
BaSO4, CaSO4
is slightly soluble.
-
Common oxides, hydroxides
and carbonates are usually insoluble (e.g. Group 2 and Transition
Metals) except those of the Group 1 Alkali Metals sodium, potassium
etc. and ammonium:
-
soluble bases–alkalis
oxides, hydroxides or carbonates: K2O, KOH, NaOH, NH3(aq), Na2CO3, (NH4)2CO3
-
insoluble bases –
basic oxides, hydroxides or insoluble carbonates: MgO, CuO, ZnO,
Mg(OH)2, Fe(OH)2, Cu(OH)2, CuCO3,
ZnCO3, CaCO3
THE METHOD
How to make an insoluble salt from
two soluble compounds (which may be a soluble salt or acid)
MAKING AN INSOLUBLE
SALT - by mixing solutions of two soluble substances
These reactions are sometimes described as a
DOUBLE DECOMPOSITION reaction
- the term is explained in examples.
-
How can we make an insoluble
salt? How do we prepare an insoluble salt from two soluble compounds?
-
This section describes the
preparation of insoluble salts like silver chloride AgCl, lead(II) chloride
(lead chloride) PbCl2, lead(II) iodide
(lead iodide) PbI2, calcium carbonate CaCO3,
barium sulfate (barium sulfate)
BaSO4,
lead(II) sulfate (lead sulfate, lead sulfate)PbSO4,
and 'slightly soluble' calcium sulfate (calcium sulfate) CaSO4,
which can all be made by a precipitation
reaction.
-
Many of the salt precipitate are WHITE, but
lead iodide is pale yellow.

Examples ...
- but it can be any soluble chloride
salt solution or even dilute hydrochloric acid (HCl). Silver nitrate is one
of the few common soluble salts of silver.
-
The silver nitrate provides the
silver ion and the sodium chloride provides the chloride ion to prepare
the insoluble salt silver chloride which forms as a
white precipitate.
-
silver nitrate + sodium chloride ==>
silver chloride + sodium nitrate
-
AgNO3(aq) + NaCl(aq)
==> AgCl(s) + NaNO3(aq)
-
In terms of
ions it could be written as
-
Ag+NO3–(aq)
+ Na+Cl–(aq) ==>
AgCl(s) +
Na+NO3–(aq)
-
or:
Ag+(aq)
+ NO3–(aq)
+ Na+(aq)
+ Cl–(aq) ==>
AgCl(s) +
Na+(aq)
+ NO3–(aq)
-
but the
spectator
ions are
nitrate NO3– and
sodium Na+
which do not change at all,
-
The 'active
ions' and resulting
precipitate are highlighted in yellow.
-
Describing this as a double
decomposition reaction:
-
In the reaction, the ions swap who they are
combined with in terms of the two ions precipitated as the salt (silver Ag+
and chloride Cl-) and the two ions left in solution (sodium Na+
and nitrate NO3-) - the silver ion is no longer with
the nitrate ion and the hydrogen ion is no longer with the chloride ion.
-
so the proper
ionic
equation is simply:
Ag+(aq)
+ Cl–(aq) ==> AgCl(s)
-
Note (i) the use of state symbols (aq) and (s) AND
-
(ii) that ionic
equations omit ions that do not change there chemical or physical
state.
-
In this case the
nitrate,
NO3–(aq) and sodium
Na+(aq)
ions do not change physically or chemically and are called
spectator ions,
-
BUT the aqueous silver
ion, Ag+(aq), combines with the aqueous
chloride ion, Cl–(aq), to form the insoluble
salt silver chloride, AgCl(s), thereby changing their
states both chemically and physically.
-
More Ionic equations explained with
all spectator ions
indicated
-
You can just use dilute hydrochloric
acid and silver nitrate solution to make insoluble silver chloride by
precipitation.
-
The silver nitrate provides the
silver ion and the hydrochloric acid provides the chloride ion to
prepare the insoluble salt silver chloride which forms as a white
precipitate.
-
silver nitrate + hydrochloric acid ==>
silver chloride + nitric acid
-
AgNO3(aq) + HCl(aq)
==> AgCl(s) +
HNO3(aq)
-
Describing this as a double
decomposition reaction:
-
In the reaction, the ions swap who they are
combined with in terms of the two ions precipitated as the salt (silver Ag+
and chloride Cl-) and the two ions left in solution (hydrogen H+
and nitrate NO3-) - the silver ion is no longer with
the nitrate ion and the hydrogen ion is no longer with the chloride ion.
-
You can apply this idea of double
decomposition to all the reactions described below.
-
In terms of
ions the reaction can be written as
-
Ag+NO3–(aq)
+ H+Cl–(aq) ==>
AgCl(s) +
H+NO3–(aq)
-
or:
Ag+(aq)
+ NO3–(aq)
+ H+(aq)
+ Cl–(aq) ==>
AgCl(s) +
H+(aq)
+ NO3–(aq)
-
BUT, the
spectator
ions are
nitrate NO3– and
hydrogen H+
which do not change at all - they remain in solution,
-
so the proper
ionic
equation is simply:
Ag+(aq)
+ Cl–(aq) ==> AgCl(s)
-
If you use barium chloride
the word and symbol equations are ...
-
barium chloride + silver
nitrate ==> silver chloride + barium nitrate
-
BaCl2(aq)
+ 2AgNO3(aq)
==> 2AgCl(s) +
Ba(NO3)2(aq)
-
which can be written as
-
Ba2+(aq)
+ 2Cl–(aq) +
2Ag+(aq) +
2NO3–(aq)
==> 2AgCl(s)
+ Ba2+(aq)
+ 2NO3–(aq)
-
the spectator ions are
Ba2+ and
NO3–
-
so the ionic equation
is: Ag+(aq)
+ Cl–(aq) ==> AgCl(s)
-
You can make silver bromide by mixing
solutions of silver nitrate and potassium bromide.
-
The silver nitrate provides the
silver ion and the potassium bromide provides the bromide ion to prepare
the insoluble salt silver bromide which forms as a cream precipitate.
-
silver nitrate + potassium bromide ==>
silver bromide + potassium nitrate
-
AgNO3(aq) + KBr(aq)
==> AgBr(s) +
KNO3(aq)
-
the
spectator
ions are
nitrate NO3– and
potassium K+
which do not change at all,
-
so the proper
ionic
equation is simply: Ag+(aq)
+ Br–(aq) ==> AgBr(s)
-
Similarly you can make silver iodide
by mixing solutions of silver nitrate and potassium iodide.
-
The silver nitrate provides the
silver ion and the potassium iodide provides the iodide ion to prepare
the insoluble salt silver iodide which forms as a pale yellow
precipitate.
-
silver nitrate + potassium iodide ==>
silver iodide + potassium nitrate
-
AgNO3(aq) + KI(aq)
==> AgI(s) +
KNO3(aq)
-
the
spectator
ions are
nitrate NO3– and
potassium K+
which do not change at all,
-
so the proper
ionic
equation is simply: Ag+(aq)
+ I–(aq) ==> AgI(s)
-
TOP OF PAGE and sub-index for page
(ii)
Lead(II) iodide,
a yellow precipitate (insoluble in water!) can be made by mixing lead(II)
nitrate solution with e.g. potassium iodide solution
- but it can be any soluble iodide salt solution mixed with lead nitrate -
one of the few common soluble salts of lead.

-
The lead nitrate supplies the
lead ion and the potassium iodide the iodide ion to make the insoluble
salt lead iodide, which is a
yellow crystalline solid.-
lead(II) nitrate + potassium
iodide ==> lead(II) iodide + potassium nitrate
-
Pb(NO3)2(aq)
+ 2KI(aq)
==> PbI2(s) + 2KNO3(aq)
-
which can be written as
-
Pb2+(aq)
+ 2NO3–(aq)
+ 2K+(aq)
+ 2I–(aq) ==>
PbI2(s) + 2K+(aq)
+ 2NO3–(aq)
-
the ionic equation is:
Pb2+(aq)
+ 2I–(aq) ==> PbI2(s)
-
because the spectator ions
are
nitrate NO3–
and
potassium K+.
-
In a similar way you can
make lead(II) chloride by e.g. using dilute hydrochloric acid
-
The hydrochloric acid supplies
the chloride ion.
-
lead(II) nitrate +
hydrochloric acid ==> lead(II) chloride + nitric acid
-
Pb(NO3)2(aq)
+ 2HCl(aq)
==> PbCl2(s) + 2HNO3(aq)
-
Pb2+(aq)
+ 2NO3–(aq)
+ 2H+(aq)
+ 2Cl–(aq) ==>
PbCl2(s)
+ 2H+(aq)
+ 2NO3–(aq)
-
the proper ionic equation is:
Pb2+(aq)
+ 2Cl–(aq) ==> PbCl2(s)
-
because the spectator
ions are nitrate NO3–
and
hydrogen H+.
-
Similarly you can
make lead(II) chloride by e.g. using dilute
sodium chloride solution
-
The silver nitrate provides the
silver ion and the sodium chloride provides the chloride ion to
prepare the insoluble salt lead chloride which forms as a white
precipitate.
-
lead(II) nitrate +
sodium chloride ==> lead(II) chloride + sodium nitrate
-
Pb(NO3)2(aq)
+ 2NaCl(aq)
==> PbCl2(s) + 2NaNO3(aq)
-
Pb2+(aq)
+ 2NO3–(aq)
+ 2Na+(aq)
+ 2Cl–(aq) ==>
PbCl2(s)
+ 2Na+(aq)
+ 2NO3–(aq)
-
the proper ionic equation is:
Pb2+(aq)
+ 2Cl–(aq) ==> PbCl2(s)
-
because the spectator
ions are nitrate NO3–
and
sodium Na+.
-
You can make
lead(II)
bromide by e.g. using sodium bromide solution
-
lead(II) nitrate +
sodium bromide ==> lead(II) bromide + sodium nitrate
-
Pb(NO3)2(aq)
+ 2NaBr(aq)
==> PbBr2(s) + 2NaNO3(aq)
-
Pb2+(aq)
+ 2NO3–(aq)
+ 2Na+(aq)
+ 2Br–(aq) ==> PbBr2(s)
+ 2Na+(aq)
+ 2NO3–(aq)
-
the proper ionic equation is:
Pb2+(aq)
+ 2Br–(aq) ==> PbBr2(s)
-
because the spectator
ions are
nitrate NO3–
and
sodium Na+.
-
The silver nitrate provides the
silver ion and the sodium bromide provides the bromide ion to
prepare the insoluble salt silver bromide which forms as a cream
precipitate.
-
You can also use potassium
bromide, just swap the Na for a K.
and you can make lead(II)
chloride by e.g. using sodium chloride solution
-
lead(II) nitrate +
sodium chloride ==> lead(II) chloride + sodium nitrate
-
Pb(NO3)2(aq)
+ 2NaCl(aq)
==> PbCl2(s) + 2NaNO3(aq)
-
Pb2+(aq)
+ 2NO3–(aq)
+ 2Na+(aq)
+ 2Cl–(aq) ==>
PbCl2(s)
+ 2Na+(aq)
+ 2NO3–(aq)
the proper ionic equation
is: Pb2+(aq)
+ 2Cl–(aq) ==> PbCl2(s)
because the spectator
ions are nitrate NO3–
and sodium Na+.
TOP OF PAGE and sub-index for page
(iii)
Calcium carbonate, a white
precipitate, forms on e.g. mixing calcium chloride solution and sodium carbonate
solutions - but it can be any soluble calcium
salt solution mixed with a solution of any soluble carbonate.

CaCl2(aq)
+
Na2CO3(aq)
==> CaCO3(s) + 2NaCl(aq)
Ca2+(aq)
+ 2Cl–(aq)
+ 2Na+(aq)
+
CO32–(aq)
==> CaCO3(s) + 2Na+(aq)
+ 2Cl–(aq)
the ionic equation is:
Ca2+(aq)
+ CO32–(aq) ==> CaCO3(s)
because the spectator ions
are
chloride Cl–
and
sodium Na+.
TOP OF PAGE and sub-index for page
(iv)
Barium sulfate
(barium sulphate), a white
precipitate, forms on mixing e.g. barium chloride solution and dilute sulfuric acid
- but it can be any soluble barium salt solution mixed with a solution of
any soluble sulfate salt solution.

BaCl2(aq)
+
H2SO4(aq)
==> BaSO4(s) + 2HCl(aq)
Ba2+(aq)
+ 2Cl–(aq)
+ 2H+(aq)
+
SO42–(aq)
==> BaSO4(s) + 2H+(aq)
+ 2Cl–(aq)
so the ionic equation is:
Ba2+(aq)
+ SO42–(aq) ==> BaSO4(s)
because the spectator ions
are
chloride Cl–
and
hydrogen H+.
-
Or you can use sulfate
salts like sodium sulfate, so the word and symbol equations are ..
-
barium chloride + sodium
sulfate ==> barium sulfate + sodium chloride
-
BaCl2(aq)
+ Na2SO4(aq)
==> BaSO4(s) + 2NaCl(aq)
-
The ionic equation is
the same:
Ba2+(aq)
+ SO42–(aq) ==> BaSO4(s)
-
because the spectator
ions are
sodium Na+
and
chloride Cl–
-
You can do exactly the
same preparation using potassium sulfate and barium nitrate or
barium chloride, basically any solutions of a soluble barium salt
and a soluble sulfate salt can be used to prepare barium sulfate.
-
e.g.
barium nitrate + potassium sulfate ==> barium sulfate +
potassium nitrate
-
or
barium chloride + potassium sulfate ==> barium sulfate +
potassium chloride
-
See at the end of the
page the uses of barium sulfate.
-
TOP OF PAGE and sub-index for page
(v)
Lead(II) sulfate
(lead sulfate), a white
precipitate, forms in a similar way e.g.
mixing lead(II) nitrate solution with sodium sulfate solution - but it
can be any soluble lead salt mixed with a solution of any soluble sulfate
salt or dilute sulfuric acid solution.
ionic equation:
Pb2+(aq)
+ SO42–(aq) ==> PbSO4(s)
because the spectator ions
are
sodium Na+
and
nitrate NO3–
Lead(II) sulfate can also be
precipitated using dilute sulfuric acid.
-
lead(II) nitrate + sodium
sulfate ==> lead(II) sulfate + nitric acid
-
Pb(NO3)2
(aq) + H2SO4(aq) ==>
PbSO4(s) + 2HNO3
(aq)
-
ionic equation:
Pb2+(aq)
+ SO42–(aq) ==> PbSO4(s)
-
because the spectator ions
are hydrogen H+
and
nitrate NO3–
ions
-
TOP OF PAGE and sub-index for page
-
(vi)
Calcium sulfate
(calcium sulfate), a white
precipitate, forms on mixing e.g. calcium chloride solution and dilute sulfuric acid
- but it can be any soluble calcium salt solution mixed with a solution of
any soluble sulfate salt.

-
calcium chloride + sulfuric
acid ==> calcium sulfate + hydrochloric acid
-
CaCl2(aq)
+
H2SO4(aq)
==> CaSO4(s) + 2HCl(aq)
-
Ca2+(aq)
+ 2Cl–(aq)
+ 2H+(aq)
+
SO42–(aq)
==> CaSO4(s) + 2H+(aq)
+ 2Cl–(aq)
-
so the ionic equation is:
Ca2+(aq)
+ SO42–(aq) ==> CaSO4(s)
-
because the spectator ions
are
chloride Cl–
and
hydrogen H+.
-
Or you can use sulfate
salts like sodium sulfate, so the word and symbol equations are ..
-
calcium chloride + sodium
sulfate ==> calcium sulfate + sodium chloride
-
CaCl2(aq)
+ Na2SO4(aq)
==> CaSO4(s) + 2NaCl(aq)
-
The ionic equation is
the same:
Ca2+(aq)
+ SO42–(aq) ==> CaSO4(s)
-
because the spectator
ions are
sodium Na+
and
chloride Cl–
You can do exactly the
same preparation using potassium sulfate and calcium nitrate or
calcium chloride, basically any solutions of a soluble calcium salt
and a soluble sulfate salt can be used to prepare and precipitate calcium sulfate.
See at the end of the
page the uses of barium sulfate.
NOTE reminder definition: A
precipitation reaction is generally defined as 'the formation of an
insoluble solid on mixing two solutions or bubbling a gas into a solution'.
TOP OF PAGE
and sub-index for page
(their preparation has been described above)
(calcium sulfate) is used in plaster of Paris and plaster for
domestic wall covering.
Barium sulfate BaSO4
(barium sulfate)
-
Barium sulfates quite a dense
material is used in with X-rays for particular medical examinations.
-
Barium sulfate, like all barium
salts is toxic, BUT, because it is insoluble, non of it is absorbed by the
body into the bloodstream and eventually it will pass right through the gut
system and be expelled in the normal faeces.
-
X-rays are used to investigate
bone structure e.g. fractured or broken bones and the technique works
because bone material is too dense to let weak X-rays through, so on
shooting an X-ray photograph you get the bone structure as a sort of shadow
effect where the X-rays have been absorbed by the bone.
-
Therefore, normally you can't
use X-rays to examine soft tissue areas like the gut.
-
However, if the patient takes a
'barium meal', a thick harmless fluid containing a suspension of the
insoluble barium sulfate, this can pass through the stomach and into the
gut.
-
Therefore it is then possible to
X-ray the intestinal gut system because the barium sulfate absorbs the
X-rays just like bone.
-
So, because barium sulfate is
opaque to X-rays, the X-ray photograph via the barium meal will highlight
the structure of the tissue lining of the gut and show up any structural
abnormalities and blockages.
TOP OF PAGE
and sub-index for page
GCSE/IGCSE foundation–easier multiple choice quiz on pH, Indicators, Acids,
Bases, Neutralisation and Salts
GCSE/IGCSE higher–harder multiple choice quiz on pH, Indicators, Acids,
Bases, Neutralisation and Salts
GCSE/IGCSE Structured question worksheet on Acid
Reaction word equations and
symbol
equation questions
Word
equation answers and
symbol
equation answers)
GCSE/IGCSE word–fill worksheet on Acids,
Bases, Neutralisation and Salts
GCSE/IGCSE
matching pair quiz on Acids, Bases, Salts and pH
See also
Advanced Level Chemistry Students Acid–Base Revision
Notes – use index
Outline the
steps in making an insoluble salt by precipitation how do you make the
insoluble salt silver bromide AgBr by precipitation? Revision KS4 Science GCSE/IGCSE/O level
Chemistry Information Study Notes for revising for AQA GCSE Science, Edexcel
Science Chemistry IGCSE Chemistry & OCR 21st Century Science Chemistry, OCR Gateway Science Chemistry,
WJEC gcse science chemistry CCEA/CEA gcse science chemistry (revise science
chemistry courses equal to US grade 8, grade 9
grade 10. Revision notes on acids, bases, alkalis, salts, solution pH word
equations balanced symbol equations science chemistry courses revision guides.
These revision notes on making salts using a precipitation reaction,
should prove useful for the new AQA chemistry, Edexcel chemistry & OCR
chemistry GCSE (9–1, 9-5 & 5-1) science courses This section describes how to make
insoluble salts: insoluble silver chloride salt AgCl,
how to make, how to make insoluble lead(II) chloride salt
(lead chloride) PbCl2, how to make insoluble lead(II) iodide salt
(lead iodide) PbI2, how do you make insoluble lead bromide PbBr2 by a
precipitation reaction how to make calcium insoluble carbonate CaCO3,
how to make insoluble barium sulfate salt (barium sulfate) BaSO4,
how to make insoluble lead(II) sulfate (lead sulfate, how to make
insoluble lead sulfate salt PbSO4, and how to make 'slightly soluble'
calcium sulfate salt CaSO4,
which can all be made by a precipitation
reaction how do you prepare insoluble salts? what do need to prepare an
insoluble salt? how do you prepare the insoluble salt lead bromide by
precipitation? what apparatus do you need to prepare an insoluble salt
by precipitation? describe a method of making an insoluble salt? GCSE
chemistry IGCSE chemistry revision notes on making insoluble salts by
precipitation KS4 GCSE Science revision notes on making insoluble salts
by precipitation GCSE chemistry guide notes on making insoluble salts by
precipitation for schools colleges academies science course tutors
images pictures diagrams for making insoluble salts by precipitation
science chemistry revision notes on making insoluble salts by
precipitation for revising chemistry module topics notes to help on
understanding of making insoluble salts by precipitation university
courses in science careers in science jobs in the industry laboratory
assistant apprenticeships technical internships USA US grade 8 grade 9
grade10 AQA chemistry science GCSE notes on making insoluble salts by
precipitation Edexcel chemistry science notes on making insoluble salts
by precipitation for OCR 21st century chemistry science notes on making
insoluble salts by precipitation OCR GCSE Gateway science chemistry
notes on making insoluble salts by precipitation WJEC gcse science
chemistry notes on making insoluble salts by precipitation CCEA/CEA gcse
chemistry notes science O level chemistry notes for making insoluble
salts by precipitation IGCSE chemistry revision notes on making
insoluble salts by precipitation O level chemistry notes how do you make
the insoluble salt silver iodide AgI by precipitation? GCSE chemistry IGCSE chemistry revision
notes on making salts by precipitation KS4 GCSE Science revision notes on
making salts by precipitation GCSE chemistry guide
notes on making salts by precipitation for schools colleges academies science course tutors images
pictures diagrams for making salts by precipitation science chemistry revision notes on
making salts by precipitation for revising chemistry module topics notes to help on understanding of
making salts by precipitation university courses in science
careers in science jobs in the industry laboratory assistant
apprenticeships technical internships USA US grade 8 grade 9 grade10 AQA
chemistry science GCSE
notes on making salts by precipitation Edexcel
chemistry science notes on making salts by precipitation for OCR 21st century chemistry science
notes on making salts by precipitation OCR GCSE Gateway science
chemistry notes on making salts by precipitation WJEC gcse science chemistry notes on
making salts by precipitation CCEA/CEA gcse
chemistry notes science O level chemistry notes for making salts
by precipitation IGCSE
chemistry revision notes on making salts by precipitation O level chemistry notes
should prove useful for the new AQA chemistry, Edexcel chemistry & OCR
chemistry GCSE (9–1, 9-5 & 5-1) science courses gcse chemistry revision
free detailed notes on making salts by precipitation to help revise igcse chemistry
igcse chemistry revision notes on making salts by
precipitation O level chemistry
revision free detailed notes on making salts by
precipitation to help revise gcse
chemistry free detailed notes on making salts by
precipitation to help revise O level
chemistry free online website to help revise making salts by
precipitation for gcse
chemistry free online website to help revise making
salts by precipitation for
igcse chemistry free online website to help revise O level
making salts by precipitation chemistry how to succeed in questions on
making salts by precipitation for gcse
chemistry how to succeed at igcse chemistry how to succeed
at O level chemistry a good website for free questions on
making salts by precipitation to help to pass gcse chemistry questions on
making salts by precipitation a good
website for free help to pass igcse chemistry with revision
notes on making salts by precipitation a good website for free help to pass O level
chemistry
TOP OF PAGE
and sub-index for page
|
 |
 |
 |
 |
 |
 |
 |
 |
 |
 |
 |
 |
 |
 |
 |
Website content © Dr
Phil Brown 2000+. All copyrights reserved on revision notes, images,
quizzes, worksheets etc. Copying of website material is NOT
permitted. Exam revision summaries & references to science course specifications
are unofficial. |
|