l ecture № 4
DESCRIPTION
L ECTURE № 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. - PowerPoint PPT PresentationTRANSCRIPT
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 preparations1. Calcium oxide (Calcii oxydum) CaО – for preparation of limy water (Aqua calcis).2. Plaster medicinal (Calcii sulfas) 2СаSО4Н2O – 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
CaCl26H2O
Calcium chloratum
CALCIUM CHLORIDE DIHYDRATE SPU, addition 1
Calcii chloridum dihydricum CaCl22H2O
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 + H2OThe 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 CaCl26H2O 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
CaCl26H2O. Crystal weight of white colour or colourless crystals.
CaCl22H2O. A crystal powder of white colour. Hygroscopic.
Solubility CaCl26H2O. Very soluble in water R, freely soluble in 96 % R.(Freezes at temperature nearby 29).CaCl2H2O. 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.
Identification1. 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: Ca2 ++ K + + [Fe (CN) 6] 4- + NH4 + KNH4Ca [Fe (CN) 6].
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 + + h1
3HNO
3HNO
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
formedСaCl2 + 2AgNO3 =2
AgCl + Сa (NO3) 2
CL - + Ag + AAgCl + 2NH4OH = [Ag (NH3) 2] Cl + 2H2O
[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 –
toxicant 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 Cr3 + + 7Н2О
2Cl - – 2е Cl2
Cr2O72– + 6Cl– + 14H+ 2Cr3+ + 3Cl2 + 7Н2О
O CNH NH C6H5
NH NH C6H5
CL2O C
N N C6H5
NH NH C6H5
CL2O C
N N C6H5
N N C6H5-2 HCl -2 HCl
+ +
diphenylcarbazide diphenylcarbazone diphenylcarbadiazone (Colourless) (orange-yellow) (violet-red)
Tests1.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 formed:
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
ASSAY1. 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 acidTitrate 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 + with Na-edetate under the scheme:
CH2 N
CH2
N
CH2COONa
CH2COOH
CH2COOH
CH2COONa
Ca
CH2COONa
CH2COOCH2 N
CH2
NCH2COO
CH2COONa
Ca2+
+ + 2 H+
Superfluous drop Na2-EDTA destroys complex CaInd, forming complex
Ca-edetat and free indicator H2Ind of dark blue colour.
Violet dark blue Em (CaCl26H2O) = М m.
CH2 N
CH2
N
CH2COONa
CH2COOH
CH2COOH
CH2COONa
Ca Ind Ca
CH2 N
CH2
NCH2COO
CH2COONa
CH2COONa
CH2COO+ + H2 Ind
+H+
Chelatomerty in the pharmaceutical analysis (SPU)Titrant – sodium EDTA (sodium salt of
ethylenediaminetetraacetate acid) (Na2-EDТА)
Test ionConditions of carrying
out of experimentIndicator mix Colouring change
Bi3 +
Solution NH3 conc.
before clouding occurrence, then HNO3 before
disappearance of clouding, t = 70 C
Xylenol orange (1 part. + 99 parts of KNO3)
pink-violet to yellow
Ca2 + Solution NаОH conc.
calconcarbonic acid
(1 part + 99 parts of NaCl)
Violet in dark blue
Mg2 +
Ammoniac buffer solution
pН 10,0, t 40 C
Eriochrome black
(1 part + 99 parts of NaCl)
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)
pink-violet
Hg2 +
Back chelatometry, excess Na2-EDТА titrate of standart
solution of ZnSO4
Eriochrome black (1 part + 99 parts of
NaCl)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) 2The superfluous drop of AgNO3 co-operates with
the indicator with formation of precipitate of orange-red colour Ag2CrО4:
2AgNO3 + K2CrО4 = Ag2CrО4 + 2KNO3Em (CaCl26H2O) = М m./2
3. Oxalic method It is based on such processes:
Quantitative precipitation of Calcium-ions:
Са2 + + С2О42–СCаС2О4 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 (CaCl26H2O) = 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 СаCl26H2O – 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 MAGNESIUM OXYDE, LIGHTSPUMagnesii oxydum leve MAGNESIUM OXYDEMagnesii oxydum MgО Маgnеsіuм oxydatumМаgnеsіа ustaNot less than 98,0 % and no more than 100,5 % MgО, in recalculation on the fried substance.
Obtaining1. Thermal processing of magnesium carbonate
basic: 3MgCO3Mg (OH) 23H2O 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) 2Fe2 + + 3ON - F e (OH) 3
And sulphatic acid H2SO4 for binding
(linkage) of Calcium-cations Ca2 +:SO4
2 - + 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 (500C) to magnesium oxide MgО:
C0500tMg (OH) 2 M gO + H2O
3. Processing of magnesium chloride superheated water steam:
MgCl2 + H2О = MgО + 2НCl
PropertiesThe 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.)
Cl4NH
N
OH
N
O Mg
N
O
2 + MgCl2
NH4OH
NH4Cl+ 2 HCl
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 theb) presence of ammonia solution and ammonium chloride
Mg2 + + HPO42 - + NH4ОН 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:
Tests
1. Inadmissible specific impurity are not present.
ASSAYShot of magnesium oxide preliminary dissolve inchloride acid dissolved R and dilute by water R:
MgO + 2HCl = MgCl2 + H2O1. 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
excess2HCl + 2NaOH = 2NaCl + 2H2O
1 mol MgО 2 mol (2 equivalent) HCl 2 mol (2 equiv.) NaOH
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 chlorideMgO + 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) NMagnesii subcarbonas
Magnesia alba Magnesium subcarbonicum
3MgCO3Mg (OH) 23H2O
t
t
Obtaining1. Interaction of solutions of magnesium sulphate and
sodium carbonate (70-80):
4MgSO4 + 4Na2CO3 + 4H2O 3MgCO3Mg (OH) 23H2O + 4Na2SO4 + CO2
2. Thermal decomposition of magnesium hydrogencarbonate:
4Mg (HCO3) 23 MgCO3Mg (OH) 23H2O + 5CO2
PropertiesThe 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)
3MgCO3Mg (OH) 23H2O + 8HCl = 4MgCl2 + 3CO2 + 8H2O
It is much easier dissolved in water which contains CO2, forming magnesium hydrogencarbonate:
3MgCO3Mg (OH) 23H2O + 5CO2 = 4Mg (HCO3) 2It 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
Identification1. 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:3MgCO3Mg (OH) 23H2O + 8HCl = 4MgCl2 + 3CO2 +
8H2O2. 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 + Н2ОВаСО3 + 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
Tests1. N. An inadmissible impurity – Barium.
Ва2 + + SO42 - B aSO4
ASSAY Shot of test substance dissolve in chloride acid хлоридной diluted R
HCl 3MgCO3Mg (OH) 23H2O + 8HCl = 4MgCl2 + 3CO2 + 8H2Osoluble 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
%100)3)(3(
)(%
223
OHOHMgMgCOm
FMgOm
.)MgO(M4
)OH3)OH(MgMgCO3(MF 223
3. Gravimetric (weight) method Shot of magnesium carbonate alkaline 3MgCO3Mg (OH) 23H2O
dry up, calcinate to constant weight and weigh (weight or gravimetric form –
MgО):
3MgCO3Mg (OH) 23H2O
= 4MgО + 3СО2 + 4Н2О
Calculate the maintenance of magnesium oxide MgО in a preparation under the formula:
,
Where F – gravimetric factor, which calculate under the formula:
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. 1Magnesii sulfas heptahydricus MAGNESIUM SULPHATE Magnesii sulfas Magnesium sulfuricum Sal amarum Bitter salt Epson salt
MgSO47H2O Not less than 99,0 % and no more than 100,5 % MgSO4 (М m. =
120,4 g/mol)
Obtaining1.Dissolution of magnesite MgCO3 a lot of hot
dissolved sulphatic acid H2SO4:
MgCO3 + H2SO4 = MgSO4 + CO2 + H2OSolution filter, evaporate before crystallisation;
thus receive epsom salt – MgSO47H2O. 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.
PropertiesThe 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.
Identification1. 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
whiteSO42 - + 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).
TestsAs magnesium sulphate MgSO47H2O 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.
ApplicationMagnesium 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 % asolution in ampoules 5, 10 or 20 ml.
MAGNESIUM CHLORIDE HEXAHYDRATE SPU, add. 1
Magnesii chloridum hexahydricum
MgCl26H2O
Not less than 99,0 % and no more than 100,5 % MgCl26H2O.
PropertiesThe description. Colourless crystals. Hygroscopic.
Solubility. Very soluble in water R, freely soluble in 96 % alcohol R.
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:
N N+
H
I
N+
SOO
O
N+
SOO
O
N+
H
CH3SO4
3 + I2 + SO2 + H2O 2 +
-+ CH3OH
The titration end define visually on change of colouring from ellow to red-brown or by 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.
Tests1. 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 precipitateASSAY
SPU. Chelatometry (see magnesium sulphate).Em (MgCl26H2O) = М m.
StorageIn the air-tight container.
MarksIn 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!