The conclusions may be summarized in the statement that the salts of strong bases with weak acids are more or less decomposed by water (hydrolyzed) and the resulting solutions must react ‹alkaline›. We find, as a matter of fact, that aqueous solutions of potassium cyanide, sodium carbonate, sodium sulphide, borax (see the table, p. 104), all react strongly alkaline to litmus (‹exp.›). Conversely, it may be said, that if the sodium or potassium salt of an acid dissolves in water with a ‹decidedly› alkaline reaction, it is the salt of a weak, poorly ionized acid.[370] [p184] «Action of Water on a Salt of a Strong Acid with a Weak Base.»—Exactly similar relations obtain in the case of salts of strong acids with weak bases:[1] they are decomposed, to a greater or less extent, into the free, strong, largely ionized acid and the free, scarcely ionized weak base, ‹the decomposition being stopped by the accumulation of the free strong acid› (more exactly, of the ‹hydrogen-ion›). Such solutions react strongly ‹acid›, as in the case of the chloride, nitrate, sulphate of aluminium, of iron (ferric), of chromium, and of similar salts of weak bases. For MeX + HOH ⇄ MeOH + HX, where MeOH ‹is a weak base› and HX a strong acid, we have as before:[371] [Me^{+}] / ([H^{+}] × [MeOH]) = [Salt] / ([Acid] × [Base]) =  K_{Base} / K_{HOH}. «Action of Water on a Salt of a Base and an Acid, Both of which are Weak.»—We will now turn to the consideration of the action of water on the fourth class of salts, the salts of a weak base with a weak acid.[372] Like all salts, such a salt, say MeX, would ionize very readily, when dissolved in water (the few exceptions to readily ionizable salts are not under consideration), and, in this case, both the positive and the negative ions would have to combine respectively with the hydroxide and the hydrogen ions of water to form the ‹nonionized weak base› and the ‹nonionized weak acid›, and satisfy ‹two very small constants›, K_{Base} and K_{Acid}: [Me^{+}] × [HO^{−}] / [MeOH] = K_{Base} and [H^{+}] × [X^{−}] / [HX] = K_{Acid}.