interest at once, and led to the concept of the combining weights
of the elements.
The first discoveries in this field were made in the last quarter of the 18th century by J. B. Richter. The point at issue was a rather commonplace one: it was the fact that when two neutral salt solutions were mixed to undergo mutual chemical decomposition and recombination, the resulting J. B. Richter’s work. liquid was neutral again, i.e. it did not contain any excess of acid or base. In other words, if two salts, A′B′ and A″ B″, composed of the acids A′ and A″ and the bases B′ and B″, undergo mutual decomposition, the amount of the base B′ left by the first salt, when its acid A′ united with the base B″ to form a new salt A′B″, was just enough to make a neutral salt A″B′ with the acid A″ left by the second salt. At first sight this looks quite simple and self-evident,—that neutral salts should form neutral ones again and not acid or basic ones,—but if this fact is once stated very serious quantitative inferences may be drawn from it, as Richter showed. For if the symbols A′, A″, B′, B″ denote at the same time such quantities of the acids and bases as form neutral salts, then if three of these quantities are determined, the fourth may be calculated from the others. This follows from the fact that by decomposing A′B′ with just the proper amount of the other salt to form A′B″, the remaining quantities B′ and A″ exist in exactly the ratio to form a neutral salt A″ B′. It is possible, therefore, to ascribe to each acid and base a certain relative weight or “combining weight” by which they will combine one with the other to form neutral salts. The same reasoning may be extended to any number of acids and bases.
It is true that Richter did not find out by himself this simplest statement of the law of neutrality which he discovered, but he expressed the same consequence in a rather clumsy way by a table of the combining weights of different bases related to the unit amount of a certain acid, and doing the same thing for the unit weight of every other acid. Then he observed that the numbers in these different tables are proportionate one to another. The same holds good if the corresponding series of the combining weights of acids for unit weights of different bases were tabulated. It was only a little later that a Berlin physicist, G. E. Fischer, united the whole system of Richter’s numbers simply into a double table of acids and bases, taking as unit an arbitrarily chosen substance, namely sulphuric acid. The following table by Fischer is therefore the first table of combining weights.
| Bases. | Acids. | ||
| Alumina | 525 | Fluoric | 427 |
| Magnesia | 615 | Carbonic | 577 |
| Ammoniac | 672 | Sebacic | 706 |
| Lime | 793 | Muriatic (hydrochloric) | 712 |
| Soda | 859 | Oxalic | 755 |
| Strontiane | 1329 | Phosphoric | 979 |
| Potash | 1605 | Formic | 988 |
| Baryte | 2222 | Sulphuric | 1000 |
| Succinic | 1209 | ||
| Nitric | 1405 | ||
| Acetic | 1480 | ||
| Citric | 1683 | ||
| Tartaric | 1694 | ||
It is interesting again to notice how difficult it is for the discoverer of a new truth to find out the most simple and complete statement of his discovery. It looks as if the amount of work needed to get to the top of a new idea is so great that not enough energy remains to clear the very last few steps. It is noteworthy also to observe how difficult it was for the chemists of that time to understand the bearing of Richter’s work. Although a summary of his results was published in Berthollet’s Essai de statique chimique, one of the most renowned chemical books of that time, nobody dared for a long time to take up the scientific treasure laid open for all the world.
At the beginning of the 19th century the same question was taken up from quite another standpoint. John Dalton, in his investigations of the behaviour of gases, and in order to understand more easily what happened when gases were absorbed by liquids, used the corpuscular hypothesis John Dalton’s atomic theory. already mentioned in connexion with Boyle. While he depicted to himself how the corpuscles, or, as he preferred to call them, the “atoms” of the gases, entered the interstices of the atoms of the liquids in which they dissolved, he asked himself: Are the several atoms of the same substance exactly alike, or are there differences as between the grains of sand? Now experience teaches us that it is impossible to separate, for example, a quantity of pure water into two samples of somewhat different properties. When a pure substance is fractionated by partial distillation or partial crystallization or partial change into another substance by chemical means, we find constantly that the residue is not changed in its properties, as it would be if the atoms were slightly different, since in that case e.g. the lighter atoms would distil first and leave behind the heavier ones, &c. Therefore we must conclude that all atoms of the same kind are exactly alike in shape and weight. But, if this be so, then all combinations between different atoms must proceed in certain invariable ratios of the weights of the elements, namely by the ratio of the weights of the atoms. Now it is impossible to weigh the atoms directly; but if we determine the ratio of the weights in which oxygen and hydrogen combine to form water, we determine in this way also the relative weight of their atoms. By a proper number of analyses of simple chemical compounds we may determine the ratios between the weights of all elementary atoms, and, selecting one of them as a standard or unit, we may express the weight of all other atoms in terms of this unit. The following table is Dalton’s (Mem. of the Lit. and Phil. Soc. of Manchester (II.), vol. i. p. 287, 1805).
Table of the Relative Weights of the Ultimate Particles of Gaseous and
other Bodies.
| Hydrogen | 1 | Nitrous oxide | 13.7 |
| Azot | 4.2 | Sulphur | 14.4 |
| Carbone | 4.3 | Nitric acid | 15.2 |
| Ammonia | 5.2 | Sulphuretted hydrogen | 15.4 |
| Oxygen | 5.5 | Carbonic acid | 15.3 |
| Water | 6.5 | Alcohol | 15.1 |
| Phosphorus | 7.2 | Sulphureous acid | 19.9 |
| Phosphuretted hydrogen | 8.2 | Sulphuric acid | 25.4 |
| Nitrous gas | 9.3 | Carburetted hydrogen from | |
| Ether | 9.6 | stagnant water | 6.3 |
| Gaseous oxide of carbone | 9.8 | Olefiant gas | 5.3 |
Dalton at once drew a peculiar inference from this view. If two elements combine in different ratios, one must conclude that different numbers of atoms unite. There must be, therefore, a simple ratio between the quantities of the one element united to the same quantity of the other. Dalton showed at once that the analysis of carbon monoxide and of carbonic acid satisfied this consequence, the quantity of oxygen in the second compound being double the quantity in the first one. A similar relation holds good between marsh gas and olefiant gas (ethylene). This is the “law of multiple proportions” (see Atom). By these considerations Dalton extended the law of combining weights, which Richter had demonstrated only for neutral salts, to all possible chemical compounds. While the scope of the law was enormously extended, its experimental foundation was even smaller than with Richter. Dalton did not concern himself very much with the experimental verification of his ideas, and the first communication of his theory in a paper on the absorption of gases by liquids (1803) attracted as little notice as Richter’s discoveries. Even when T. Thomson published Dalton’s views in an appendix to his widely read text-book of chemistry, matters did not change very much. It was only by the work of J. J. Berzelius that the enormous importance of Dalton’s views was brought to light.
Berzelius was at that time busy in developing a trustworthy
system of chemical analysis, and for this purpose he investigated
the composition of the most important salts. He then
went over the work of Richter, and realized that by his
law he could check the results of his analyses. He tried
Work of
J. J.
Berzelius.
it and found the law to hold good in most cases; when
it did not, according to his analyses, he found that the error was
on his own side and that better analyses fitted Richter’s law.
Thus he was prepared to understand the importance of Dalton’s
views and he proceeded at once to test its exactness. The result
was the best possible. The law of the combining weights of the
