LECTURE № 4
Theme: Inorganic metal-containing
compounds of Calcium, Magnesium,
Zinc, Copper and Bismuth as drugs
Associate prof. Mosula L.M.
The plan
1. Inorganic drugs of Calcium.
2. Inorganic drugs of Magnesium.
3. Inorganic drugs of Zinc.
4. Inorganic drugs of Copper.
5. Inorganic drugs of Bismuth.
Inorganic drugs of Calcium
Biological action and medical
application
Ions Са2 + – formation of bone and
tooth tissue; strengthen ability to live of
cages; promote reduction
of skeletal muscles and heart muscles;
curlings of blood necessary for
improvement.
Calcium preparations
1. Calcium oxide (Calcii oxydum) CaО – for
preparation of limy water (Aqua calcis).
2. Plaster medicinal (Calcii sulfas)
2СаSО4Н2O – for surgery.
3. Calcium a carbonate precipitated (Calcii
carbonas praecipitatus) СаСО3-at the raised
acidity of gastric juice.
4. Calcium chloride crystal (we will consider in
more details).
5. Organic preparations of Calcium (calcium
lactate, calcium gluconate, calcium
glycerophosphate) will be considered in following
lectures.
CALCIUM CHLORIDE HEXAHYDRATE
SPU, addition 1
Calcii chloridum hexahydricum
CaCl26H2O
Calcium chloratum
CALCIUM CHLORIDE DIHYDRATE
SPU, addition 1
Calcii chloridum dihydricum
CaCl22H2O
Calcium chloratum
Not less than 97,0 % and no more than 103,0 %
of corresponding substances.
Obtaining
1. Marble processing by chloride acid:
CaCO3 + 2HCl = CaCl2 + CO2 + H2O
The received solution concentrate and clear calcium chloride
CaCl2
of impurity (Fe2 + and Mg2 +) action of chloride acid HCl
(FeCl2 and MgCl2)
Elimination: a solution sate with chlorine Cl2:
FeCl2  FeCl3
Precipitation FeCl3 and MgCl2 by
hydrated lime Ca (OH) 2:
2FeCl3 + 3Ca (OH) 2 = Fe (OH) 3 + 3CaCl2
MgCl2 + Ca (OH) 2 = Mg (OH) 2 + CaCl2
Filter
The solution is enriched CaCl2.
Excess of hydrated lime Ca (OH) 2
delete action of chloride acid HCl:
Ca (OH) 2 + 2HCl = CaCl2 + 2H2O
Calcium chloride hexahydricum CaCl26H2O is crystallize
out.
2. From solutions which are formed as a waste at
soda reception
on Solve method (CaCl2 – a unique by-product in this
method).
Properties (SPU, addition 1)
The description
CaCl26H2O. Crystal weight of white
colour or colourless crystals.
CaCl22H2O. A crystal powder of
white colour. Hygroscopic.
Solubility
CaCl26H2O. Very soluble in
water R, freely soluble in 96 %
R.
(Freezes at temperature nearby
29).
CaCl2H2O. Freely soluble in
water Р, soluble in 96 % R.
Because of the big hygroscopicity in
drugstores prepare 50 %
a solution (Calcium chloratum
solutum 50 %), and from
this concentrate prepare necessary
drugs which contain calcium chloride.
Identification
1. Reactions for Calcium-ions Са2 + (see lime chloride, lecture 1
a) SPU. Interaction with a alcoholic solution of
glyoxalhydroxyanil in the
alkaline medium in the presence of chloroform;
chloroformic layer is painted
in red colour at the expense of
formation of intracomplex compound
with Calcium, which extract by chloroform:
b) SPU. Interaction solution of a preparation in
acetic acid
with potassium ferrocyanide (II) К4 [Fe (CN) 6] at presence
of ammonium chloride NH4Cl; the white crystal precipitate of
ammonium-potassium-calcium ferrocyanide (II), insoluble in
acetic acid СН3СООН is formed:
c) SPU, N. Reaction with ammonium oxalate (NH4) 2C2O4
the white precipitate,
insoluble in dissolved acetic acid СН3СООН and a solution
of ammonia R, soluble in the dissolved mineral acids is formed:
Ca2 + + C2O42 - CaС2O4.
d) SPU, N: Pirochemical reaction. The salt of Calcium
wetted with chloride acid R and brought in a colourless flame,
paints it in orange-red colour.
Са2 + + h *Са2 + Са2 + + h1
NO
3 
2. Reactions for chlorides-ions Cl - (acid chloride see, lecture 1)
a) SPU. Reaction with a solution silver nitrate in
the presence of nitric acid; the white curdled precipitate is formed
СaCl2 + 2AgNO3 =2
AgCl + Сa (NO3) 2
CL - + Ag + A
NO 3 AgCl + 2NH OH = [Ag (NH ) ] Cl + 2H O
4
3 2
2


[Ag (NH3) 2] Cl + HNO3 = AgCl + 2NH4NO3
b) Action of oxidizers (К2Cr2O7 (SPU)), in the
presence of sulphatic acid; gas chlorine Cl2 is allocated (to smell it is impossible –
xicant gas!):
b) Action of oxidizers (К2Cr2O7 (SPU)), in the presence of
sulphatic acid;
gas chlorine Cl2 is allocated (to smell it is impossible –
toxicant gas!):
3СаCl2 + K2Cr2O7 + 7H2SO4 = 3Cl2 + Cr2 (SO4) 3 + 3СаSO4 +
К2SO4 + 7H2O
Cr2O72 - + 14H + + 6е 2Cr3 + + 7Н2О
2Cl - – 2е Cl2
Cr2O72– + 6Cl– + 14H+  2Cr3+ + 3Cl2 + 7Н2О
NH
O
NH
C
NH
NH
C6H5 + CL
2
C6H5 -2 HCl
diphenylcarbazide
(Colourless)
N
O
N
C6H5
+ CL2
C
NH
NH
C6H5 -2 HCl
diphenylcarbazone
(orange-yellow)
O
N
N
C6H5
N
N
C6H5
C
diphenylcarbadiazone
(violet-red)
Tests
1. Aluminium (an inadmissible impurity).
2. To solution S add a solution of ammonium chloride R,
solution of ammonia dissolved R1 and heat up to boiling;
the solution should not cloud and the precipitate should not be form
Al3+ + 3NH4OH  Al(OH)3 + 3NH4+
2. Barium (an inadmissible impurity).
To solution S add a solution calcium of sulphate R;
opalescence the received solution is not more intense
than that in a mix of solution S and water:
Ва2 + + SO42 -  ВaSO4
ASSAY
1. SPU. Chelatometry, direct titration
Titrant – a standard solution of sodium EDTA
(ethylenediaminetetraacetate acid) (Na2–EDTA)
Medium– the concentrated solution of
sodium hydroxide NаOH
Indicator – indicator mix of calconcarbonic acid
Titrate test solution before change
of colouring with violet to dark blue.
Chemism:
At addition to test solution of calcium chloride of indicator mix
of
calconcarbonic acid H2Ind (dark blue colouring) the
complex metal-indicator CaInd (red-violet colour) is formed:
CaCl2
+ H2Ind
=
CaInd + 2HCl
dark blue
violet.
At titration of such solution by standard solution Na-edetate
in the environment of the concentrated solution sodium
hydroxide NаOH (рН 7)
is formed very strong colourless soluble in water a complex of
ions Са2 +
CH2COONa
CH2COONa
H2C with
N Na-edetate under
H2C N
the scheme:
+
2+
Ca
CH2COOH
+
C N
H2
CH2COOH
CH2COONa
CH2COO
C N
H2
CH2COO
CH2COONa
Ca
+
2H
Superfluous drop Na2-EDTA destroys complex CaInd,
forming complex
Ca-edetat and free indicator H2Ind of dark blue colour.
H2C N
Ca Ind
Violet
+
CH2COONa
CH2COONa
+ H2C N
CH2COOH +H
CH2COO
CH2COOH
C N
CH2COONa
H2
CH2COO
Ca
+ H2 Ind
C N
CH2COONa
H2
Em (CaCl26H2O) = М m.
dark blue
Chelatomerty in the pharmaceutical analysis (SPU)
Titrant – sodium EDTA (sodium salt of
ethylenediaminetetraacetate acid) (Na2-EDТА)
Test ion
Bi3 +
Conditions of carrying
out of experiment
Indicator mix
Solution NH3 conc.
before
clouding
Xylenol orange
occurrence,
then
(1 part. +
HNO3
before
99
parts
of
disappearance
of
KNO3)
clouding,
t = 70 C
Ca2 +
Solution NаОH conc.
calconcarbonic
acid
(1 part + 99
parts of NaCl)
Mg2 +
Ammoniac buffer
solution
pН 10,0, t = 40 C
Eriochrome
black
(1 part + 99 parts
of NaCl)
Colouring change
pink-violet to yellow
Violet in dark blue
Violet in dark blue
Pb2 +
hexamethylenetetramine (the
alkaline medium) pH~7,8–8,2
Xylenol orange
(1 part + 99 parts of
NaCl)
Violet-red in
the yellow
Zn2 +
hexamethylenetetramine (the
alkaline medium) pH~7,8–8,2
Xylenol orange
(1 part. + 99 parts of
KNO3)
Violet-red in
the yellow
Al3 +
Back chelatometry, excess
Na2-EDТА titrate of standart
solution
of Pb (NO3) 2
Xylenol orange
(1 part. + 99 parts of
KNO3)
Hg2 +
Back chelatometry, excess
Na2-EDТА titrate of standart
solution
of ZnSO4
Eriochrome black
(1 part + 99 parts of
NaCl)
pink-violet
The violet
2. Argentometry (Моrh method), direct titration
Titrant – a standard solution of silver nitrate AgNO3;
Medium – neutral (!)
Indicator – a solution of potassium chromate K2CrО4.
Titrate before occurrence of orange-red colour of precipitate
1СаCl2 + 2AgNO3 = 2AgCl + Сa (NO3) 2
The superfluous drop of AgNO3 co-operates with
the indicator with formation of precipitate of
orange-red colour Ag2CrО4:
2AgNO3 + K2CrО4 = Ag2CrО4 + 2KNO3
Em (CaCl26H2O) = М m./2
3. Oxalic method
It is based on such processes:
Quantitative precipitation of Calcium-ions
Са2 + + С2О42–СCаС2О4
Precipitate dissolution in
dissolved sulphatic acid H2SO4
СаС2О4 + 2Н+  Са2+ + Н2С2О4;
Titration oxalate acid Н2С2О4, which was
formed
(its quantity is equivalent to an investigated
preparation of Calcium),
by standard solution of potassium permanganate
KMnO4
2KMnО4 + 5Н2С2О4 + 3H2SO4 = 2MnSO4 + 10CO2
+ K2SO4 + 8H2O
MnО4–+ 8H + + 5 e Mn2 + + 4H2O | 5 | 2
H2С2O4 – 2e 2СО2 + 2H + | 2 | 5
5H2С2O4 + 2MnО4– + 6H+  2Mn2+ + 10СО2 +
8H2O
Em (CaCl26H2O) = М m./2
Storage. In the air-tight container.
Store in a dry place, in the glasswares which
stoppers fill in with paraffin,
considering high hygroscopicity. Therefore in drugstores prepare
a concentrate – 50 % a solution
(Calcium chloratum solutum 50 %)
which cultivation receive solutions of
a preparation of necessary concentration.
Marks. In necessary cases mark:
the substance is
suitable for manufacture of
solutions for a dialysis.
Application, Anti-inflammatory, antiallergic,
hemostatic means.
Accept oral or enter intravenously
on 5–15 ml of 10 %
of a solution (contains СаCl26H2O – 100 ml,
waters for injections – to 1L).
At introduction hypodermically or
intramuscularly causes necrosis tissue (!).
Inorganic drugs of Magnesium
MAGNESIUM OXYDE, HEAVY
SPU
Magnesii oxydum ponderosum
SPU
Magnesii oxydum leve
Magnesii oxydum
MAGNESIUM OXYDE, LIGHT
MAGNESIUM OXYDE
MgО
Маgnеsіuм oxydatum
Маgnеsіа usta
Not less than 98,0 % and no more than 100,5 % MgО,
in recalculation on the fried substance.
Obtaining
1. Thermal processing of magnesium carbonate
basic:
3MgCO3Mg (OH) 23H2O 4
t


MgО + 3CO2 + 4H2O
t 250–300 C.
2. From a brine (pickle) at processing of
potash salts which contain MgCl2
a) To a brine add limy milk Ca (OH) 2 for
sedimentation of impurity Fe2 + and Fe3 +:
Fe2 + + 2ON -  F e (OH) 2
Fe2 + + 3ON -  F e (OH) 3
And sulphatic acid H2SO4 for binding
(linkage) of Calcium-cations Ca2 +:
SO42 - + Ca2 +  C aSO4
b) Excess of limy milk Ca (OH) 2 binding of
magnesium chloride MgCl2 in a kind magnesium
hydroxide Mg (OH)2:,
MgCl2 + Ca (OH) 2 = Mg (OH) 2 + CaCl2
c) Calcination of magnesium hydroxide (500) C)
to magnesium oxide MgО:
Mg (OH) 2
M gO + H2O
3. Processing of magnesium
chloride superheated water steam:
MgCl2 + H2О = MgО + 2НCl
t = 500 0 C


Properties
The description (SPU)
Magnesium oxide heavy is fine powder of white colour.
Magnesium oxide light – finel amorphous powder
of white colour.
Solubility. Are practically insoluble in water R,
in which find out alkaline reaction with phenolphthalein.
(Are soluble in the dissolved acids.)
Identification
Reactions for Magnesium-ions Mg2 + (after dissolution substance
in nitric acid dissolved R HNO3
and neutralisations by a solution sodium гидроксида dissolved Р NаOH).
MgО + 2HNO3 = Mg (NO3) 2 + H2O
a) SPU. Reaction with sodium hydrogenphosphate in the
b) presence of ammonia solution and ammonium chloride
Mg2 + + HPO42 - + NH4ОН
NH Cl
4

NH4MgPO4 + Н2О
white precipitate
b) Reaction with 8-oxyquinoline in the medium of an ammoniac buffer solution;
the yellow- green crystal precipitate of magnesium 8-oxyquinoline is formed:
+
2
N
OH
NH4OH
MgCl2
+
NH4Cl
N
O
N
Mg
O
2 HCl
Tests
1. Inadmissible specific impurity are not present.
ASSAY
Shot of magnesium oxide preliminary dissolve in
chloride acid dissolved R and dilute by water R:
MgO + 2HCl = MgCl2 + H2O
1. SPU. Chelatometry, direct titration (see the table
Em (MgО) = М m.
2. The acid-base titration, back titration
In the presence of methyl orange colouring before
transition from pink to the yellow.
1MgО + 2HCl = MgCl2 + H2O
excess
2HCl + 2NaOH = 2NaCl + 2H2O
1 mol MgО 2 mol (2 equivalent) HCl 2 mol (2 equiv.) NaO
Therefore Em (MgO) = М m./2
Storage. In densely corked container.
Application. Antiacid agent.
MgO neutralizes chloride acid of gastric
juice, magnesium
oxide turns in magnesium chloride
MgO + 2HCl = MgCl2 + H2O
which finds out laxative effect.
The release form: a powder and tablets
for 0,5 g.
Is a part of preparations of “Almagel”,
“Gastal”, and also an antidote at a
poisoning with acids.
MAGNESIUM CARBONATE, HEAVY
SPU, add. 1
Magnesii subcarbonas
ponderosus
MAGNESIUM CARBONATE, LIGHT
SPU, add. 1
Magnesii subcarbonas levis
MAGNESIUM CARBONATE ALKALINE (BASIC) N
Magnesii subcarbonas
Magnesia alba
Magnesium subcarbonicum
3MgCO3Mg (OH) 23H2O
Obtaining
1. Interaction of solutions of magnesium sulphate and
sodium carbonate (70-80):
4MgSO4 + 4Na2CO3 + 4H2O 3
t
MgCO3Mg (OH) 23H2O + 4Na2SO4 + CO2

2. Thermal decomposition of magnesium
hydrogencarbonate:
t
4Mg (HCO3) 2 
3 MgCO3Mg (OH) 23H2O + 5CO2
Properties
The description
SPU, add. 1. A powder of white colour.
Solubility
SPU, add. 1. It is practically insoluble in water R.
(It is dissolved in the dissolved acids with
rough allocation of bubles of gas)
3MgCO3Mg (OH) 23H2O + 8HCl = 4MgCl2 + 3CO2 + 8H2O
It is much easier dissolved in water which contains
CO2, forming magnesium hydrogencarbonate:
3MgCO3Mg (OH) 23H2O + 5CO2 = 4Mg (HCO3) 2
It is possible to express this process
to such simplified equations:
MgCO3 + H2O + CO2 = Mg (HCO3) 2
Therefore magnesium hydrogencarbonate is a
component of many mineral waters.
At standing a transparent solution magnesium
hydrogencarbonate
again cloud as a result of decomposition reaction:
Mg(HCO3)2  MgCO3 + H2O + CO2
Identification
1. SPU, add. 1. Bulk volume
15 g substances of magnesium carbonate heavy are
occupied with volume about 30 ml.
15 g substances of magnesium carbonate light are
occupied with volume about 180 ml.
Test for identity of magnesium carbonate
of the core spend:
3MgCO3Mg (OH) 23H2O + 8HCl = 4MgCl2 + 3CO2 + 8H2O
2. Reactions for Magnesium-ions Mg2 +
(after preliminary dissolution in the dissolved acids)
(see magnesium oxide).
3. Reactions for carbonate-anions СО32–:
a) SPU, interaction with mineral acids (SPU – acetic acid
dissolved R СН3СООН):
СО32– + 2СН3СООН = 2СН3СОО– + Н2О + СО2
Gas, which is allocated (without colour and a smell),
pass through a solution barium hydroxide R Ва (OH)2;
the white precipitate, which is dissolved a lot of chloride acid R1 HCl is formed.
СО2 + Ва (OH) 2 = ВаСО3 + Н2О
ВаСО3 + 2HCl = BaCl2
b) SPU, N. Reaction with the sated solution of magnesium sulphate
At addition to a water solution of a substance, which contains anions of СО32–
sated solution of magnesium sulphate R MgSO4 at room temperature
is formed white precipitate MgCO3 (difference hydrogencarbonate,
which form a precipitate only at boiling):
CO32 - + Mg2 + = MgCO3
Tests
1. N. An inadmissible impurity – Barium.
Ва2 + + SO42 -  B aSO4
ASSAY
Shot of test substance dissolve in chloride acid хлоридной diluted R HCl
3MgCO3Mg (OH) 23H2O + 8HCl = 4MgCl2 + 3CO2 + 8H2O
soluble with water R and spend quantitative definition (MgCl2)
similarly magnesium oxide (see above).
1. SPU. Chelatometry, direct titration
(see magnesium oxide)
As the preparation structure is not constant,
recalculation do on the maintenance magnesium oxide MgО.
Em (MgО) =М. M.
2. The acid-base titration, back titration
(similarly magnesium oxide).
Em (MgО) = М m./2
3. Gravimetric (weight) method
Shot of magnesium carbonate alkaline 3MgCO3Mg (OH) 23H2O dry up
, calcinate to constant weight and weigh (weight or gravimetric form – MgО):

3MgCO3Mg (OH) 23H2O
= 4MgО + 3СО2 + 4Н2О
Calculate the maintenance of magnesium oxide MgО in a preparation under the formula:
% =
,
m( MgO )  F
100%
m(3MgCO3  Mg (OH ) 2  3H 2O)
Where F – gravimetric factor, which calculate under the formula:
M(3MgCO3  Mg(OH) 2  3H 2O)
F=
.
4M( MgO )
Maintenance МgO should be less than 40,0 % and no more than 45 %.
Storage. In densely corked container.
Application. Antiacid agent.
Release forms: a powder and tablets
which contain magnesium
carbonate alkaline (0,5 g) and
sodium a hydrocarbonate (0,5 g).
Is a part of tablets “Vicalinum”,
“Vicairum”.
MAGNESIUM SULPHATE
HEPTAHYDRATE
SPU, add. 1
Magnesii sulfas heptahydricus
MAGNESIUM SULPHATE
Magnesii sulfas
Magnesium sulfuricum
Sal amarum
Bitter salt
Epson salt
MgSO47H2O
Not less than 99,0 % and no more than 100,5 % MgSO4 (М m. = 120,4
g/mol)
Obtaining
1. Dissolution of magnesite MgCO3 a lot of hot dissolved
sulphatic acid H2SO4:
MgCO3 + H2SO4 = MgSO4 + CO2 + H2O
Solution filter, evaporate before crystallisation;
thus receive epsom salt
– MgSO47H2O. The filtered crystals recrystallization from
water.
Properties
The description. SPU, add. 1. A crystal powder of white
colour
or brilliant colourless crystals.
Solubility. SPU, add. 1. Freely soluble in water R,
very soluble in boiling water R, it is practically
insoluble in 96 % alcohol R.
Properties
The description. SPU, add. 1. A crystal powder of
white colour or brilliant colourless crystals.
Solubility. SPU, add. 1. Freely soluble in water R,
very soluble in boiling water R, it is practically
insoluble in 96 % alcohol R.
Identification
1. Reactions for Magnesium-ions Mg2 + (see magnesium
oxide):
2. Reactions for sulphate-anions SO42 –
(see sodium sulphate, lecture 2):
a)SPU. Reaction with solution of barium chloride
ВаCl2 in chloride-acid medium HCl;
white precipitate ВаSO4 is formed:
MgSO4 + BaCl2 = BaSO4 + MgCl2
white
SO42 - + Ва2 +  ВаSO4
The white precipitate is insoluble in mineral acids and alkalis.
SPU. To the suspension, received in reaction a),
add a solution of iodine I2; yellow colouring does not disappear
(difference from sulphites SO32 - and dithionites S2O32–),
but becomes colourless at addition by drops of solution
tin (ІІ) chloride SnCl2 (difference from iodates IO3–).
A mix boil; the deposit does not become colourless
(difference from selenates and wolframates):
MgSO4 + I2 (iodine does not become colourless).
I2 + SnCl2 + 4HCl = 2HI + H2 [SnCl6] (iodine becomes colourless).
Tests
As magnesium sulphate MgSO47H2O apply
for parenteral introductions, and also inside and in
considerable quantities therefore especial requirements
to its cleanliness are put.
1. Solution S. The substance solution in water R
2. should be clear and colourless.
2. Acidity or alkalinity.
ASSAY
SPU. Chelatometry (see magnesium oxide)
Em (MgSO4) = М m.
Storage. In hermetically corked container
because easily disappears.
Application
Magnesium sulphate has versatile influence on an organism.
1. At intake as a laxative.
2. At parenteral introduction - restful action on
the central nervous system.
3. In the form of 25 % of a solution enter
hypodermically as antispasmodic.
4. Apply to a labour pain relief, as
anticonvulsant intramuscularly on 5–20 ml of
25 % of a solution.
In case of redispensing of magnesium sulphate enter
intravenously 10 % a solution of calcium chloride
(antagonists).
Release forms: a powder, 20 % or 25 % a
solution in ampoules 5, 10 or 20 ml.
MAGNESIUM CHLORIDE HEXAHYDRATE
SPU, add. 1
Magnesii chloridum hexahydricum
MgCl26H2O
Not less than 99,0 % and no more than 100,5 % MgCl26H2O
Properties
The description. Colourless crystals. Hygroscopic.
Solubility. Very soluble in water R, freely soluble in 96 % alcohol
Identification
1. Definition of water by semimicromethod (Fisher's method).
Iodometric definition of a moisture. The maintenance of water from 51,0
% to 55,0 %. Fisher's reagent is a solution of sulphur dioxide SO2, iodine
I2 and pyridine C5H5N in a methanol. At the heart of a method oxidation
SO2 by means of iodine I2 in the presence of water lays:
SO2 + I2 + 2Н2О  H2SO4 + 2HI
Reaction needs to be spent at presence pyridine, which as the mild base ,
connects (binds) HI and SO2 in nonvolatile compounds:
+ I2 + SO2 + H2O
3
N
I +
2
+
+
N
H
N
O
S
O
O
-
+ CH3OH
+
+
N
O
S
O
CH3SO4
N
H
O
The titration end define visually on change of colouring from ellow to red-brown or b
means of potentiometry.
2. Reactions for Magnesium-ions Mg2 + (see magnesium oxide):
3. Reactions for chlorides-ions Cl - (see calcium chloride):
a) SPU. Reaction with a solution of silver nitrate in the presence
of nitric acid; the white curdled precipitate is formed;
b) SPU. Action of potassium dichromate К2Cr2O7
in the sulphatic-acid medium;
gas chlorine Cl2 which paints the filtering paper
moistened of diphenylcarbazide, in violet-red colour is allocated.
Tests
1. Solution S prepared by dissolution test substance in water,
free from СО2, R, should be clear and colourless.
2. Acidity or alkalinity.
4. Potassium. (not more than 500 ppm).
5. Aluminium. (not more than 1 ppm).
6. N. An inadmissible impurity – Barium:
Ва2 + + SO42 -  BaSO4
white precipitate
ASSAY
SPU. Chelatometry (see magnesium sulphate).
Em (MgCl26H2O) = М m.
Storage
In the air-tight container.
Marks
In necessary cases mark:
The substance is suitable for manufacture of solutions for
perenteral dialysis, a hemodialysis or a haemofiltration;
The substance is suitable for manufacture of drugs
for parenteral applications.
 Thanks
for attention!