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The principal period groups were digitalis preparations, squill, broom, juniper oil, buchu, nitrous ether spirit, and several soluble potassium salts. They were grouped by observed promotion of urine flow, rather than by one common mechanism. The following are historical adult quantities per administration, expressed in the contemporary units; they are not present-day prescriptions.

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Other recognised period agents included dandelion and copaiba. The dandelion decoction was given in quantities of 1–2 fluid ounces, its soft extract in quantities of 10–30 grains, and its preserved juice in quantities of ½–2 fluid drachms. Copaiba was given in quantities of 15–30 minims, and copaiba oil in quantities of 5–20 minims. Their historical inclusion does not establish that they are suitable substitutes for current diuretic therapy. ^[ref]

The distinction between preparations matters more than a single “dose of the plant”: an infusion, tincture, juice and powder have different concentrations. Likewise, a salt's small historical diuretic dose is not its larger purgative dose. A modern explanation also separates a direct effect on renal tubules from improved cardiac output in appropriate heart failure: digitalis preparations cannot be understood simply as agents that make every kidney excrete more water. Modern digoxin is used for selected cardiac indications, rather than as a general treatment for low urine output. ^[ref]

Oxygen can be obtained by decomposing an oxygen-rich chemical compound, or by separating it from air. For the historical laboratory, heating potassium chlorate, heating certain metal oxides, and electrolysis of water are useful examples. The substance collected is molecular oxygen, ${\mathrm{O}}_2$.

A common preparation heats potassium chlorate, often with manganese dioxide as a catalyst:A heat-resistant vessel and delivery tube conduct the evolved gas to an inverted collecting vessel over water, after the initial displaced air has been excluded. Oxygen is only slightly soluble in water, making this collection principle useful. The manganese dioxide changes the reaction rate and required heating conditions; it is not the net source of the oxygen in this catalysed balance. Without the catalyst, potassium perchlorate can occur as an intermediate.

Two older preparations use heated metal oxides:The first explains the historical decomposition of mercury(II) oxide, with metallic Mercury deposited on cooler parts of the apparatus. It is historical chemistry, not a preferred present-day teaching preparation. The second is one stage in the reduction of manganese dioxide; at still higher temperature further oxygen loss can give ${\mathrm{Mn}}_3{\mathrm{O}}_4$, so the oxide residue depends on the conditions. Strong heating of potassium nitrate provides another net balance:In electrolysis, suitable separated electrodes collect oxygen at the anode and hydrogen at the cathode. With a suitable electrolyte and electrodes, the net chemical equation isThe gases must be kept in separate collecting spaces if the experiment is to demonstrate their separate identities and the approximately $2:1$ volume ratio. Choice of electrolyte matters: a chloride-containing electrolyte can give chlorine instead of clean oxygen evolution.

For a modern small-scale comparison, catalytic decomposition of hydrogen peroxide givesThis is a different feedstock from potassium chlorate. Large-scale separation of oxygen from air by cryogenic fractionation belongs to later industrial practice and should not be substituted for an 1866 laboratory answer. A collected sample can be tested by its vigorous support of combustion, conventionally the relighting of a glowing splint; this observation identifies a property, while the preparation and exclusion of interfering gases establish the sample's provenance.