Codex @codex  0

The source may be a pipe, cistern, service connection or fitting. Robert Christison's pre-examination experiments addressed the action of different waters on metallic lead: very pure waters, including distilled water or rainwater, could attack it, whereas salts in many natural waters modified the process. This provides a contemporary basis for treating the character of the supply, as well as the material of the cistern or pipe, as important.^[ref]

The dissolving tendency is called plumbosolvency. In modern chemical terms, low pH and low alkalinity can favour the release of lead. Dissolved oxygen supports corrosion of the metal; dissolved carbon dioxide affects both acidity and carbonate chemistry. Carbonate deposits can provide a partly protective surface layer, while conditions favouring their dissolution can increase release. It is therefore misleading to say simply that all carbon dioxide prevents contamination or that all waters containing it dissolve lead to the same degree. Water hardness and alkalinity are related features of many waters but are not interchangeable quantities.^[ref]

Long contact, especially stagnation overnight or through disuse, can increase contamination. Warmer conditions, changes in the supply chemistry, disturbance of an old pipe and the condition of accumulated deposits can also matter. Water can carry dissolved lead or particles containing lead; an old apparently coated pipe is not an assurance that release has ceased. Modern supplies may additionally encounter lead-bearing solder or brass, which should be recognized as a present comparison rather than assumed to be the construction of a particular 1864 installation.^[ref]

A clear appearance and acceptable taste cannot exclude lead. Investigate the actual plumbing materials and analyse appropriately collected samples, recording the period of standing and other conditions instead of inventing a concentration. The most direct way to remove the source is replacement of lead-bearing components; treatment that controls corrosion is chemistry-dependent and is not equivalent to a universal guarantee from a hard-water scale. These considerations answer when contamination is likely without imposing an unsupported period numerical threshold.

The 1864 preparations contain either crude opium or its aqueous Extractum Opii; those quantities must be distinguished from a quantity of isolated morphine. The following are the officinal opium preparations. Ratios for solids mean the mass fraction in the compounded preparation; liquid strengths specify mass per volume or the actual ingredients used.

The arithmetic uses the new avoirdupois ounce of 437.5 grains, not the old apothecaries' ounce of 480 grains. These are historical formulation proportions, not modern assays of morphine delivered after solvent extraction. Confectio Opii was omitted in 1864, and this edition's Vinum Opii contains no spices. The separate morphine hydrochloride preparations—Liquor Morphiae Hydrochloratis, Suppositoria Morphiae, Trochisci Morphiae, and Trochisci Morphiae et Ipecacuanhae—contain an isolated alkaloid salt rather than crude opium. ^[ref]

The seven named mixtures of the 1864 British Pharmacopoeia are Mistura Ammoniaci, Mistura Amygdalae, Mistura Creasoti, Mistura Cretae, Mistura Ferri Composita, Mistura Guaiaci and Mistura Scammonii. Their compositions are as follows; avoirdupois ounces are used for solids and fluid ounces for liquids.

The category is an official preparation name, not every possible bedside combination of medicines. Camphor water and acacia mucilage are not additional entries under Mistura: the 1864 names are Aqua Camphorae and Mucilago Acaciae. ^[ref]

Pulvis Jalapae Compositus contains powdered jalap 5 avoirdupois ounces, potassium hydrogen tartrate 9 avoirdupois ounces, and powdered ginger 1 avoirdupois ounce. Thus the mass proportions are 5:9:1, and jalap supplies one third of the powder's mass. This is a compound purgative, not pure jalap resin. ^[ref]

Pilula Scillae Composita contains powdered squill 1¼ avoirdupois ounces, powdered ginger, ammoniacum and hard soap 1 avoirdupois ounce each, with treacle 2 avoirdupois ounces, or sufficient to make a pill mass. Using the specified 2 avoirdupois ounces of treacle, the whole is 6¼ avoirdupois ounces and contains one fifth squill by mass. The allowance of sufficient treacle makes consistency a compounding requirement, not a claim that every moist pill batch has an analytically exact 20% squill content. ^[ref]

Liquor Morphiae Hydrochloratis contains morphine hydrochloride 4 grains, dilute hydrochloric acid 8 minims, rectified spirit 2 fluid drachms and distilled water 6 fluid drachms. Its conventional strength is ½ grain of morphine hydrochloride per fluid drachm, not ½ grain of free morphine. The small quantity of hydrochloric acid maintains an acid solution. ^[ref]

Liquor Strychniae contains strychnine 4 grains, dilute hydrochloric acid 6 minims, rectified spirit 2 fluid drachms and distilled water 6 fluid drachms. Dissolve the strychnine in the acid mixed with part of the water, using the prescribed assistance of heat, then add the spirit and remaining water. Its conventional strength is ½ grain of strychnine per fluid drachm. Acid promotes solubility by forming a soluble salt of the alkaloid. ^[ref]

For the last two solutions, the stated historical strengths use the nominal 8 fluid drachms of spirit and water. The extra few minims of dilute acid must still appear in the actual recipe; treating all ingredient volumes as perfectly additive would not give an exact modern analytical concentration.

The 1864 iron list includes metallic, ferrous, ferric and compound preparations; its wet Ferri Peroxidum Hydratum was used historically as an antidote to arsenic poisoning. It must be distinguished from dried Ferri Peroxidum and from later editions' reassignment of similar Latin names.

The officinal articles and preparations are:

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Prepare the hydrated peroxide by inducing precipitation from the ferric solution with sodium hydroxide, collecting and washing the wet precipitate, and preserving it without drying in a covered vessel. The starting solution is Liquor Ferri Persulphatis, whose “persulphate” here means ferric sulfate, not a modern peroxydisulfate salt. Add the appropriately diluted ferric solution to the alkaline liquor with stirring, allow the precipitate to settle, collect it on a calico filter, and wash with distilled water until the washings no longer give a precipitate with barium chloride. This tests removal of soluble sulfate. The resulting fresh, hydrated material is kept wet; drying gives the separate dried preparation. ^[ref]

In modern chemical notation the precipitation can be idealised asThe fresh solid is a hydrated ferric oxide material with variable water content; the equation is not a claim that every pharmaceutical batch is one pure, crystalline iron hydroxide. Its historical use depended on binding dissolved arsenic into less available material in the digestive tract, especially the freshly precipitated, wet state. It was not a universal antidote to every metal or every stage of absorbed arsenic poisoning. Contemporary discussion explicitly identified the new hydrated peroxide as an arsenic antidote. ^{[ref] [ref]}

Modern treatment of significant arsenic poisoning concerns systemic toxicity and may involve specialist-directed chelation therapy; a nineteenth-century ferric paste is not the modern treatment standard. ^[ref]

Prepare quinine sulfate by acidic extraction of cinchona bark, alkaline precipitation of the quinine base, conversion into the sulfate, and purification by crystallization. “Quinia” is the historical name for quinine.

The 1867 process starts with one pound of yellow cinchona bark in coarse powder, three fluid ounces of hydrochloric acid, four pints of solution of sodium hydroxide, and sufficient distilled water and diluted sulfuric acid. The hydrochloric acid is diluted with ten pints of distilled water. The bark is first moistened with diluted sulfuric acid, macerated for twenty-four hours with occasional stirring, and then exhausted in a percolator with the diluted hydrochloric acid. The historical endpoint is disappearance of the bitter character of the emerging liquid. This describes the period's test, not an instruction to taste an unidentified medicinal material.^[ref]

The soluble alkaloid salts enter the percolate. Adding solution of sodium hydroxide liberates the much less water-soluble quinine base. After settling, the liquid is decanted and the precipitate collected on a filter and washed with cold distilled water until the washings cease to be coloured. The precipitate is then treated warm with distilled water and diluted sulfuric acid, added gradually to obtain a neutral liquid with nearly all the precipitate dissolved. The hot solution is filtered through paper, the filter washed with distilled water, and the filtrate concentrated until a surface film appears. It is then set aside for crystallization; the crystals are dried on filter paper without applied heat. This is a separation of a naturally occurring alkaloid, not a synthesis of the quinine skeleton.

Writing $B$ for the quinine base, the central changes are:The successive changes in solubility explain the apparatus: a percolator washes soluble salts out of the powder; a filter retains the liberated base; a heated porcelain vessel dissolves the crude base as its sulfate; cooling then recovers the less soluble crystals. Other cinchona alkaloids can accompany the product, which is why appearance and bitterness are insufficient evidence of purity.

The 1867 “Characters and Tests” combine identity and purity checks. They must be read as a group:

The historical quantity and endpoint requirements belong to the 1867 monograph.^[ref] Its formula represents the then-described heptahydrate; the current “Quinine sulfate” instead specifies a dihydrate and modern tests for related cinchona alkaloids. The modern specification explains that distinction; the exam's historical tests remain those listed above.^[ref]