lecture № 3 inorganic drugs with acid-base properties. inorganic official compounds of carbon,...

LECTURE № 3

Inorganic drugs with acid-base

properties. Inorganic official compounds

of Carbon, Aluminium, Barium, Silver,

which are used in the medical practice

Associate prof. Mosula L.M.

The plan

1. Inorganic acids as drugs: Hydrochloric acid, Boric acid.

2. Borax - pharmacopoeial preparation of sodium salt of boric

acid.

3. Pharmacopoeial preparations of Ammonia: Strong ammonia

solution, Dilute ammonia solution.

4. Sodium Bicarbonate.

5. Inorganic drugs of Carbon: Activated Charcoal , Sodium

bicarbonate.

6. Inorganic drug of Aluminium: Dried Aluminium hydroxide.

7. Inorganic drug of Barium: Barium sulphate.

8. Inorganic drug of Silver: Silver nitrate.

Browse: British Pharmacopoeia 2009

SPU, add. 1

British Pharmacopoeia Volume I & II

Monographs: Medicinal and Pharmaceutical Substances

Hydrochloric Acid

Hydrochloric AcidGeneral Notices

(Concentrated Hydrochloric Acid, Ph Eur monograph 0002)

Acidum hydrochloriсum

Аcidum muriaticum

HCl

36.46 7647-01-0

DEFINITION

Content

35.0 per cent m/m to 39.0 per cent m/m.

35.0 per cent m/m to 39.0 per cent m/m.

OBTAINING

General industrial method for obtaining hydrogen chloride is synthesis from

gases hydrogen H2 and chlorine Cl2. This gases is obtained by electrolysis water

solution of sodium chloride: (in the solution is ions of Na+ and Cl–, and dipoles

of water Н2О):

Cathode (–): Na+; Н2О 2Н2О + 2е 2ОН– + Н2 (reduction)

Anode (+): Cl– ; Н2О 2Cl– – 2e Cl2 (oxidution)

General reaction:

2NaCl + 2HOH H2 + Cl2 + 2NaOH

cathode anode

Obtained gases to burn in the contact furnace:

Н2 + Сl2 = 2НCl

Obtained gas (HCl) to pass through absorption tower with water - hydrogen

chloride (HCl –gas) freely soluble in water, and formed Hydrochloric acid with

concentration 35–37 %, it is fuming hydrochloric acid. Saturated at t =18 С

solution of Hydrochloric acid has 42 % gas hydrogen chloride.

CHARACTERS

Appearance

Clear, colourless, fuming liquid.

Solubility

Miscible with water.

Relative density

About 1.18.

IDENTIFICATION

A. (BrPh, SPU, add. 1). Dilute with water R. The solution is strongly acid (2.2.4).

Tabl. Relationship between reaction of solution, Approximate ph and colour of

certain.

B. (BrPh, SPU, add. 1). It gives the reactions of chlorides (2.3.1).

HCl + AgNO3 → AgCl↓ + НNO3;

Cl– + Ag+ → AgCl↓

AgCl↓ + 2NH4OH → [Ag(NH3)2]Cl + 2H2O.

B. (BrPh, SPU). Reaction with potassium dichromate in the sulphuric -acid

medium.

Э14HCl + K2Cr2O7 = 3Cl2 + 2CrCl3 + 2KCl + 7H2O

Cr2O72– + 14H+ + 6е 2Cr3+ + 7Н2О

2Cl– – 2е Cl2

diphenylcarbazide diphenylcarbazone diphenylcarbadiazone

(colourless) (orange-yellow) (violet-red)

C. (BrPh, SPU, add. 1). It complies with the limits of the assay.

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

+ +

ASSAY

(BrPh, SPU, add. 1). Alkalimetry, direct titration

HCl + NaOH = NaCl + H2O

Еm(HCl) = M. m.

STORAGE

In a stoppered container made of glass or another inert material, at a

temperature not

exceeding 30 °C.

Preparation

Dilute Hydrochloric Acid

Ph Eur

Browse: British Pharmacopoeia 2009 SPU, add 1





General Notices

(Ph Eur monograph 0003)

Acidum hydrochloricum dilutum

HCl

DEFINITION

Content

9.5 per cent m/m to 10.5 per cent m/m of HCl (Mr 36.46).

PREPARATION

To 726 g of water R add 274 g of concentrated hydrochloric acid and mix.

IDENTIFICATION the same as Concentrated Hydrochloric Acid.

ASSAY

Alkalimetry, direct titration

Action and use

Agent, which regulated metabolic processes. 0,3–0,5 % HCl use at insufficient

gastric acidity.

Browse: British Pharmacopoeia 2009 SPU



Boric Acid

Boric Acid

General Notices


Acidum boricum

H3BO3

61.8ээ10043-35-3

Ph Eur

DEFINITION

Content

99.0 per cent to 100.5 per cent.

OBTAINING

Interaction hot hydrochloric acid (or sulphuric acid) with tetraborates (borax

Na2B4O710H2O or boron-calcite СаB4O74H2O) (for medicinal purposes):

Na2B4O710H2O + 2HCl = 4Н3ВО3 + 2NaCl + 5H2O

СаB4O74H2O + 2HCl + Н2О = 4Н3ВО3 + СаCl2

Na2B4O7 + H2SO4 + 5H2O = 4Н3ВО3 + Na2SO4

CHARACTERS

Appearance

White or almost white, crystalline powder, colourless, shiny plates greasy to the

touch, or white or almost white crystals.

Solubility

Soluble in water and in ethanol (96 per cent), freely soluble in boiling water and in

glycerol (85 per cent).

IDENTIFICATION

эA. (BrPh, SPU). Bromomethyl ester formation. Dissolve 0.1 g by gently heating in 5 ml

of methanol R, add 0.1 ml of sulphuric acid R and ignite the solution. The flame has a green

border.

Н3ВО3 + 3СН3ОН (СН3О)3В + 3Н2О

B. (BrPh, SPU). Interaction with indicators. Solution S (see Tests) is acid (2.2.4).

ASSAY

(BrPh, SPU). Alkalimetry, direct titration. Dissolve 1.000 g with heating in 100 ml of

water R containing 15 g of mannitol R. Titrate with 1 M sodium hydroxide, using 0.5 ml of

phenolphthalein solution R as indicator, until a pink colour is obtained.

1 ml of 1 M sodium hydroxide is equivalent to 61.8 mg of H3BO3.

NaOH + Н3ВО3 = NaВО2 + 2H2O

NaВО2 + 2H2O = Н3ВО3 + NaOH.

If titrate only with 1 M sodium hydroxide without mannitol R then the medium becomes alkaline before end

point that is drug substance is titrated not completely.

For intensification of acid properties of boric acid add polyatomic alcohol - mannitol (hexatomic alcohol, it

formatted with boric acid complex compound. Then the complex compound titrate with 1 M sodium hydroxide:

Em (Н3ВО3) = М.m.

Action and use. Antiseptic agent.

CH2OH

HHO

HHO

OHH

OHH

CH2OH

H3BO3H

+

CH2OH

HHO

HHO

OHH

OH

CH2O

CH2OH

OHH

OHH

HHO

HO

CH2OB

NaOH

Na+

CH2OH

HHO

HHO

OHH

OH

CH2O

CH2OH

OHH

OHH

HHO

HO

CH2OB

H2O.+ 2

_

+- 3H2O

_

Browse: British Pharmacopoeia 2009 SPU



Borax

BoraxGeneral Notices

Sodium Borate; Sodium Tetraborate


Natrii tetraboras

Natrium tetraboriсum

Na2B4O7,10H2Oэ

э381.4ээ1303-96-4

Ph Eur

DEFINITION

Disodium tetraborate decahydrate.

Content

99.0 per cent to 103.0 per cent of Na2B4O7,10H2O.

CHARACTERS

Appearance

White or almost white, crystalline powder, colourless crystals or crystalline

masses,

efflorescent.

Solubility

Soluble in water, very soluble in boiling water, freely soluble in glycerol.

IDENTIFICATION

A. (BrPh, SPU). Bromomethyl ester formation.

B. (BrPh, SPU). Action the water solution of borax on indicators. To 5 ml of solution S

add 0.1 ml of phenolphthalein solution R. The solution is red. On the addition of 5 ml of

glycerol (85 per cent) R the colour disappears.

Water solution of borax owing to hydrolysis has the alkaline reaction (pН 7):

Na2B4O7 + 7HOH = 2NaOH + 4H3BO3 pН = 9,0 - 9,6

At addition glycerol to water solution of borax there is formation boron-glyceric acid and the

solution has acid reaction of medium (colouring of phenolphthalein solution disappears):

C. (BrPh, SPU). Solution S gives the reactions of sodium (2.3.1).

CH2OH

CHOH

CH2OH

CH2OH

CH

H2C O

OB

O CH

CH2O

HOCH2

HOH

BOH

OH+ ++2 3 H2O

Na2B4O7Na

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OH

H2C OH H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

H

H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

+ ++

27H2O

8

+

1 моль 2

+

H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

H NaOH

H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

Na+

2 mol

+ ++ 2 H2O222

ASSAY

(BrPh, SPU). Alkalimetry mannitol solution of borax.

Em(Na2B4O7∙ 10H2O) = M.m./2

STORAGE. Protected from air.

Action and use. Antiseptic agent.

Na2B4O7Na

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OH

H2C OH H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

H

H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

+ ++

27H2O

8

+

1 mol 2

+

H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

H NaOH

H2C O

CH2

CH

CH

OH

OH

OH

CH

CH

OH

OB

CH2

CH

CH

CH

CH

OH

OH

OH

O

OH

CH2O

Na+

2 mol + +

+ 2 H2O222


?



Dried Aluminium Hydroxide

Dried Aluminium Hydroxide

General Notices

(Hydrated Aluminium Oxide, Ph Eur monograph 0311)

Aluminii hydroxydum

Al(OH)3

Algeldratum*

Argilla pura

Aluminium hydroxydatum

DEFINITION

Content

47.0 per cent to 60.0 per cent of Al2O3 (Mr 102.0).

CHARACTERS

Appearance

White or almost white, amorphous powder.

Solubility

Practically insoluble in water. It dissolves in dilute mineral acids and in solutions of

alkali

hydroxides.

IDENTIFICATION

(BrPh, SPU). Solution S (see Tests) gives the reaction of aluminium (2.3.1).

Aluminium Salts

Dissolve about 15 mg of the substance to be examined in 2 ml of water R or

use 2 ml of the prescribed solution. Add about 0.5 ml of dilute hydrochloric acid R and

about 0.5 ml of thioacetamide reagent R. No precipitate is formed. Add dropwise

dilute sodium hydroxide solution R. A gelatinous white precipitate is formed

which dissolves on further addition of dilute sodium hydroxide solution R. Gradually

add ammonium chloride solution R. The gelatinous white precipitate is re-

formed.

Al(OH)3 + 3HCl = AlCl3 + 3H2O

solution

AlCl3 + 3NaOH = Al(OH)3 + 3NaCl

gelatinous

white precipitate

Al(OH)3 + 3NaOH = Na3[Al(OH)6]

precipitate dissolves

Na3[Al(OH)6] + 3NH4Cl = Al(OH)3 + 3NaCl + 3NH4OH

gelatinous

white precipitate is re-formed

ASSAY

(BrPh). Chelatometry, back titration.

Other method – Gravimetry.

Shot of test substance of Al(OH)3 dry, fry to constant mass and lower (weight or

gravimetric form – Al2O3):

2Al(OH)3 Al2O3 + 3Н2О

Calculate content clear Al(OH)3 in the preparation by formula:

, there

F – gravimetric factor, calculate by formula:

STORAGE

In an airtight container , at a temperature not exceeding 30 °C.

Action and use

Antacid.

Preparations

Aluminium Hydroxide Tablets

Co-magaldrox Oral Suspension

Co-magaldrox Tablets

Compound Magnesium Trisilicate Tablets

Ph Eur

%100))OH(Al(m

F)OAl(m%

3

32

.)(

)((2

32

3

OAlM

OHAlMF

Browse: British Pharmacopoeia 2009b SPU, add. 1



Barium Sulphate

Barium Sulphate

General Notices


Barii sulfas

Barii sulfas pro roentgeno

Barium sulfuricum pro roentgeno

BaSO4

ээ233.4ээ7727-43-7

OBTAINING

1. From nature mineral barite ВаSО4

Stages:

а) Barite ВаSО4 reduction by coal С at fry to barium sulphide ВаS:

BaSO4 + 2С = ВаS + 2CO2

б) Processing by hydrochloric acid HCl; soluble salt of barium chloride BaCl2 is

formed:

BaS + 2HCl = H2S + BaCl2

в) Precipitation of BaSO4 by sodium sulphate Na2SO4, or magnesium sulphate

MgSO4 or sulphatic acid H2SO4:

BaCl2 + Na2SO4 BaSO4 + 2NaCl

That BaSO4 will be superfine, solutions must be very dilute, and beside, add protective

colloid (linseed or linseed mucilage) for slowly precipitation of BaSO4.

Precipitate of BaSO4 screen wash by water (for inadmissible impurities of Chlorides:

soluble salt BaCl2 is toxic). Thus wash off and impurities of Sulphates SO42–.

CHARACTERS

Appearance

Fine, white or almost white powder, free from gritty particles.

Solubility

Practically insoluble in water and in organic solvents. It is very slightly soluble in

acids and in

solutions of alkali hydroxides.

IDENTIFICATION

эA. (BrPh, SPU, add. 1). Boil a suspension of 0.2 g with 5 ml of a 500 g/l solution

of sodium carbonate R for 5 min, add 10 ml of water R, filter and acidify a part of

the filtrate with dilute hydrochloric acid R. The solution gives the reactions of

sulphates (2.3.1).

BaSO4 + Na2CO3 BaCO3 + Na2SO4

carbonization white

precipitate on the filter

Sulphates

A. (BrPh, SPU). Reaction with barium chloride solution in the hydrochloric-acid

medium. Dissolve about 45 mg of the substance to be examined in 5 ml of water

R or use 5 ml of the prescribed solution. Add 1 ml of dilute hydrochloric acid R

and 1 ml of barium chloride solution R1. A white precipitate is formed.

Na2CO3 + 2HCl = NaCl + H2O + CO2

Na2SO4 + BaCl2 = BaSO4 + 2NaCl

white precipitate

B. (BrPh).B. (BrPh). To the suspensionTo the suspension obtained during reaction (a), obtained during reaction (a), addadd 0.1 ml of 0.1 ml of 0.05 M 0.05 M

iodineiodine. The . The suspension remains yellowsuspension remains yellow (distinction from sulphites and dithionites), but (distinction from sulphites and dithionites), but

is decolorised by adding dropwise is decolorised by adding dropwise stannous chloride solution stannous chloride solution RR (distinction from (distinction from

iodates). iodates). Boil the mixture. No coloured precipitate is formedBoil the mixture. No coloured precipitate is formed (distinction from (distinction from

selenates and tungstates).selenates and tungstates).

B. (BrPh, SPU, add. 1). Reaction with sulphuric acid. B. (BrPh, SPU, add. 1). Reaction with sulphuric acid. Wash the residue Wash the residue

collected in the preceding test with 3 successive small quantities of collected in the preceding test with 3 successive small quantities of water Rwater R. To the . To the

residue add 5 ml of residue add 5 ml of dilute hydrochloric acid Rdilute hydrochloric acid R, filter and add to the filtrate 0.3 ml of , filter and add to the filtrate 0.3 ml of dilute dilute

sulphuric acid Rsulphuric acid R. A . A white precipitate is formedwhite precipitate is formed that is insoluble in that is insoluble in dilute sodium dilute sodium

hydroxide solution Rhydroxide solution R..

BaCO3 + 2HCl = BaCl2 + H2O + CO2BaCO3 + 2HCl = BaCl2 + H2O + CO2

BaCl2+ H2SO4 = BaCl2+ H2SO4 = BaSO4BaSO4 + 2HCl + 2HCl

white precipitatewhite precipitate

OTHER REACTION:OTHER REACTION:

Pyrochemical reaction. All salts of Barium burns a yellow-green colour. Pyrochemical reaction. All salts of Barium burns a yellow-green colour.

2. Reaction with solution of potassium chromate 2. Reaction with solution of potassium chromate K2CrK2CrОО44 or potassium or potassium

dichromate dichromate K2Cr2O7; yellow precipitate of BaCrK2Cr2O7; yellow precipitate of BaCrОО4 is formed:4 is formed:

Ba2+ + CrBa2+ + CrОО42–42– = BaCr = BaCrОО44

ASSAY in the Pharmacopoeia is not presents.

Not Pharmacopoeial method – Ion-exchange chromatography.

Heating BaSO4 in the water at t 70–80 С with ion-exchange resin

H-type (cation exchanger) during 12 hour. Occurrence cation

exchange: cations of Barium Ba2+ adsorbs on cation exchanger, in

the filtrate occurres equivalent quantity of sulphuric acid:

BaSO4 + 2H- cation exchanger Ba- cation exchanger + H2SO4\

H2SO4, which formed in the filtrate, titrate with 0,1 М sodium

hydroxide NaOH, as indicator use phenolphthalein and titrate until

occirence pink colour.

H2SO4 + 2NaOH = Na2SO4 + 2H2O

Em(BaSO4 ) = М. m./2

Action and use

Radio-opaque substance used in the investigation of the gastro-

intestinal tract.

Preparation

Barium Sulphate for Suspension.

Ph Eur

Browse: British Pharmacopoeia 2009 SPU, add. 1



Silver Nitrate

Silver Nitrate

General Notices


Argenti nitras

Argentum nitricum

Lapis infernalis

AgNO3

ээ169.9ээ7761-88-8

DEFINITION

Content

99.0 per cent to 100.5 per cent.

OBTAINING

1. Dilution Silver in the 25% solution of nitric acid:

3Ag + 4HNO3 = 3AgNO3 + NO + 2H2O

2. Dilution Cu-Al alloy in the nitric acid at heating:

AgCu + 4HNO3 AgNO3 + Cu(NO3)2 + NO + 2H2O

Obtained Silver nitrate is nessesery to clear from impurities.

CHARACTERS

Appearance

White or almost white, crystalline powder or transparent, colourless crystals.

Solubility

Very soluble in water, soluble in ethanol (96 per cent).

IDENTIFICATION

A. (BrPh, SPU). 10 mg gives the reaction of nitrates (2.3.1).

Nitrates :

Reaction with nitrobenzene in the presence of sulphuric acid. To a mixture of 0.1 ml of

nitrobenzene R and 0.2 ml of sulphuric acid R, add a quantity of the powdered substance

equivalent to about 1 mg of nitrate (NO3–) or the prescribed quantity. Allow to stand for 5 min. Cool

in iced water and add slowly and with mixing 5 ml of water R, then 5 ml of strong sodium hydroxide

solution R. Add 5 ml of acetone R. Shake and allow to stand. The upper layer is coloured deep

violet.

Not pharmacopoeial reactions:

1. Interaction with diphenylamine in the acid medium (conc. H2SO4) with formation

organic dye dark blue colour (analogical to Nitrites-ions, see NaNO2):

diphenylbenzidine

sulphoimmonium salt of diphenylbenzidine (dye with dark blue colour)

2. Interaction with iron(ІІ) sulphate solution FeSO4 in the concentrated sulphatic-acid

medium H2SO4; brown ring (FeSO4NO) is formatted (in the clock glass):

2NaNO3 + 6FeSO4 + 4H2SO4 = 2NO + 3Fe2(SO4)3 + Na2SO4 + 4H2O

NO + Fe2+ + SO42– [Fe(NO)]SO4

This reaction is possible to make in the tube: to solution of drug add conc. H2SO4, then add

iron(ІІ) sulphate solution FeSO4. On the joint two liquids dark-brown ring of unstable compound

FeSO4NO is formed.

Chemism:

2AgNO3 + H2SO4 = Ag2SO4 + 2HNO3

HNO3 + 3H2SO4 + 6FeSO4 = 3Fe2(SO4)3 + 2NO + 4H2O

FeSO4 + NO = FeSO4NO

B. (BrPh, SPU). 10 mg gives the reaction of silver (2.3.1).

Silver and Silver Compounds:

Reaction with hydrochloric acid. Dissolve about 10 mg of the substance to be examined

in 10 ml of water R or use 10 ml of the prescribed solution. Add 0.3 ml of hydrochloric acid

R1. A curdled, white precipitate is formed that dissolves on addition of 3 ml of dilute

ammonia R1.

AgNO3 + HCl = AgCl + HNO3

AgCl + 2NH4OH = [Ag(NH3)2]Cl + 2H2O

From all insoluble halogenides of Silver only for AgCl is characteristic solution in

the ammonium carbonate (NH4)2CO3 :

AgCl + (NH4)2CO3 = [Ag(NH3)2]Cl + H2O + CO2

Not pharmacopoeial reactions:

1. Reaction of “silver mirror”

At addition to ammoniac solution of silver nitrate AgNO3 (Tolens reagent)

formaldehyde solution and heating after fixed time on the tube wall metallic silver scurf in

the form of “silver mirror” is formed:

2AgNO3 + 2NH4OH = [Ag(NH3)2]NO3 + 2H2O

HCНO + 2[Ag(NH3)2]NO3 + H2O = 2Ag + HCOONH4 + NH3 + 2NH4NO3

2. Reaction with potassium chromate solution

At addition to silver nitrate solution AgNO3 solution of potassium chromate K2CrО4

orange-red precipitate of silver chromate Ag2CrО4, is formed. This precipitate is soluble in

the HNO3 and NH4OH, almost insoluble in the CH3COOH:

AgNO3 + K2CrО4 = Ag2CrО4 + 2KNO3

ASSAY

(BrPh, SPU, add. 1). Thiocyanatometry, direct titration. Dissolve 0.300 g in 50

ml of water R, add 2 ml of dilute nitric acid R and 2 ml of ferric ammonium sulphate

solution R2. Titrate with 0.1 M ammonium thiocyanate until a reddishyellow colour is

obtained.

1 ml of 0.1 M ammonium thiocyanate is equivalent to 16.99 mg of AgNO3.

AgNO3 + NH4SCN = AgSCN + NH4NO3

3NH4SCN + FeNH4(SO4)2 = Fe(SCN)3 + 2(NH4)2SO4

Em (AgNO3) = M.m.

STORAGE

In a non-metallic container, protected from light.

Ph Eur

Action and use

Antiseptic.

Preparation

Sterile Silver Nitrate Solution

Ph Eur




Colloidal Silver for External Use

Colloidal Silver for External Use

General Notices


ээээ9015-51-4

Action and use

Antibacterial.

Ph Eur

DEFINITION

Colloidal metallic silver containing protein.

Content

70.0 per cent to 80.0 per cent of Ag (dried substance).

CHARACTERS

Appearance

Green or bluish-black metallic shiny flakes or powder, hygroscopic.

Solubility

Freely soluble or soluble in water, practically insoluble in ethanol (96 per cent) and in

methylene chloride.

STORAGE

In an airtight container .

Ph Eur

Inorganic preparations of Carbon

Carbon - main component of vegetative and animal organisms. In

earth crust and the nature meets as in a free kind (graphite, diamond), it is

artificial origin - carbin (in USSR) and bakebol (USA), and as a part of

minerals - carbonates: CaCO3 - calcite; MgCO3 - magnesite;

CaCO3ЧMgCO3 - dolomite; FeCO3 - siderite, iron spar; (CuOH) 2CO3

- malachite. In air 0,03 % of carbonic gas CO2 contain.

In medical practice apply absorbent coal (coal activated), sodium

hydrocarbonate, carbon (IV) oxide..

Activated charcoal Carbo activatus СObtaining

Coal - a product of decomposition of organic substances.

1. Coal of an animal origin - Carbo animalis, bone coal

(roasting bones of animals), blood coal (blood roasting). Such coal

contains to 80 % of ashes (mineral salts, Сa3 (PO4) 2) and only

7-10 % of coal ©. For clearing of coal of an animal origin from

ashes, process it the acids, which excess wash away water, and

then dry. After such processing animal coal already contains of

ashes only 5-6 % and to 90 % C, shows high adsorption ability.

2. Coal of a phytogenesis (vegetable origin) (charcoal)

obtain pyrolysis of wood of hardwood of trees without air access.

Such coal has a small amount of ashes (to 6 %), therefore does

not require additional processing, as coal of an animal origin.

3. Absorbent coal (Coal activated). For obtaining of coal

activated, applied in medicine, wood or animal coal to processing

superheated water steam (at 100 °С). Thus a time pores is cleared of

resinous impurities, the internal surface considerably increases and

consequently increases adsorption ability. One g coal has an

internal surface to 1000 m2; an ultrapores in diameter

approximately 10-9 m playing an active role in the process of

adsorption; a micropores in diameter 10-3-10-5 m). It adsorbs

on the surface various substances, in particular heavy

metals, phenols, spirits, dyes etc.

Adsorption ability can be increased, adding a debonder

(process of solution ZnCl2, MgCl2, NaOH or H3PO4 with the

subsequent heating to 300-400 °С); thus water steam (H2O)

reacts with the added substances (ZnCl2, MgCl2) with

formation of gas HCl which disappears and loosens coal,

increasing a surface of a pores.

Properties

Coal activated represents a black powder without

a smell and taste. It is insoluble in water and other

solvents.

High quality

The coal activated contains impurity ZnO, MgO.

Also the maintenance of impurity of chlorides Cl -

sulphates SO42–, heavy metals, Fe, As is regulated.

There should not be impuriy of sulphides S2–,

carbonates СО32–, cyanides CN–

(inadmissible impurity).

Their revealing:

Application. Adsorbing means.

Apply as adsorbing means at food intoxications (sausage

poison, mushrooms) and at diseases of a gastroenteric path

(at the raised acidity and fermentation in a stomach) - doses

0,5-1 g 3-4 times a day, and also at poisonings of alkaloids,

salts of heavy metals - doses 20-30 g on (single, one-time) in

the form of a suspension in water.

Release forms

Tablets of coal activated Tabulеttae Carbonis

actiwati 0,25 aut 0,5.

Consist: coal activated - 0,25 or 0,5 g

Auxiliary substances - enough.

Tablets – Carbolenum. (73% C, 10%sugar, 12% starch, 5% NaCl).

Sodium hydrocarbonateNatrii hydrocarbonas

NaHCO3

Natrium hydrocarbonicum Natrium bicarbonicumBaking soda

HO

NaOC O

Obtaining 1. Rose's method (1801): interaction of carbonic gas CO2 with crystal soda Na2CO3

.10 H2O:

Na2CO3.10 H2O + CO2 → NaHCO3 + 9H2O

2. Leblan's method (french a doctor, 1791): obtaining of soda from sodium chloride NaCl, however it is polluted by impurity of chlorides, calcium sulphide CaS and demands corresponding clearing.

2. Solve's ammoniac method (belgian engineer, 1863, more economic method): the concentrated solution of sodium chloride NaCl sate with ammonia NH3 at cooling and simultaneously under pressure pass through it carbonic gas CO2:

NH3 + CO2 + H2O = NH4HCO3 NH4HCO3 + NaCl = NH4Cl + NaHCO3

Properties

The description. White crystal powder without a smell, the

salty-alkaline taste, steady in a dry premise, slowly decays in damp

air. At heating to 270 °С with formation carbonate sodium

completely decays:2NaHCO3 → Na2CO3 + CO2+ H2O

Therefore weight loss at calcining (frying), makes not

less than 36,6 % (CO2+ H2O).

At temperature 70 °С in a water solution double salt

Na2CO3*NaHCO3 is formed, and at 100 °С - Na2CO3.

.

Solubility. Soluble in water, practically insoluble in 95

% alcohol. Water solutions have alkalescent reaction (рН =

8,37), caused by salt hydrolysis:

NaHCO3 + НОН NaОН + CO2+ H2O HCO3 – + НОН ОН– + Н2CO3

Identification1. Reactions of Na+ (see NaF)

2. Reactions of hydrocarbonate-ion HCO3–:

а) SPU. Interaction with acetic acid СН3СООН

NaHCO3 + СН3СООН = СН3СООNa + CO2↑ + H2O CO2 + Ва(ОН)2 = BaCO3↓ + H2O

BaCO3 + 2HCl = BaCl2 + CO2 + H2O

b) SPU, N. Reaction with saturated solution of magnesium sulphate MgSO4 at the boiling:

2NaHCO3 → Na2CO3 + CO2 + H2O 4MgSO4 + 4Na2CO3 + 4H2O =

3MgCO3.Mg(ОН)2

.3H2O↓ + 4Na2SO4 + CO2 c) SPU, N Solution colouring by means of phenolphtalein. To a water

solution of a preparation add a solution of phenolphtalein; the solution remains

colourless or becomes poorly pink (difference from the carbonates which solutions get

red colouring).

By means of reactions is possible in the conditions of a drugstore to

distinguish hydrocarbonates from carbonates.

ASSAY. Acidimetry, direct titration T – standart solution of HClInd – methyl orangeTitrate until pink colour. NaHCO3 + HCl = NaCl + CO2 + H2O

Em(NaHCO3) = M.м.

If in a preparation there is an impurity of sodium carbonate

Na2CO3 results will be overestimated.

Storage. In well corked banks, in a cool and dry place. Under the

influence of damp air passes in sodium a carbonate.

Application. Antiacid agent.

Apply sodium a hydrocarbonate in quality antiacid agent at the raised

acidity of gastric juice, a stomach ulcer of a stomach and duodenum..

However at neutralization of hydrochloric acid carbonic gas which again

stimulates secret allocation is allocated. Therefore it accept together with

enveloping and adsorbing substances which reduce this collateral action.

Accept inside in mixtures in quality expectorant in powders (0,5-1 g)

some times in day.

outwardly apply in the form of 0,5-2 % of water solutions to inhalations,

washings, rinsings a nose, stomatitises, a laryngitis. Use 2 %-s' solution of

baking soda for washing of eyes and mucous membrane of the top

respiratory ways at hit on them of acids.

At expressed acidosis enter intravenously - 50-100 ml 3-5 % solutions.

Release forms: a powder, tablets of sodium of hydrocarbonate

Tabulettes Natrii hudrocarbonas 0,3 aut 0,5; a solution of sodium of

a hydrocarbonate 5 %-s' for injection, suppository - 0,3, 0,5 and 0,7 g.

Thanks for attention!

lecture № 3 inorganic drugs with acid-base properties. inorganic official compounds of carbon,...

Documents

solution of hydrochloric

reaction of solution

sulphuric acid medium

acidbase properties

gas hcl

inorganic drug of aluminium

inorganic drug of silver

inorganic drug of barium