Most solubility references (e.g. this one) say that there are "few" insoluble salts of alkali metals.
Are there any exceptions?
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2$\begingroup$ Though I don't know the details, some types of uranium ions can precipitate sodium and ammonium cations when added to water as their respective diuranates. If I recall correctly, a qualitative method to identify sodium in aqueous solution is to add potassium uranyl sulphate in the absence of any other non-group 1 cations. I'm curious what other insoluble salts exist, especially for the heavier alkalis. $\endgroup$ – Nicolau Saker Neto Feb 22 '14 at 23:04
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$\begingroup$ chemistry.stackexchange.com/questions/82328/… $\endgroup$ – Nilay Ghosh Jul 14 '18 at 17:14
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$\begingroup$ The link given is dead. Please update. $\endgroup$ – Oscar Lanzi Jun 30 at 14:37
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Lithium carbonate has poor water solubility. Cesium triphenylcyanoborate is insoluble in water.
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They would advertise $\ce{NaBPh4}$ as a reagent to determine $\ce{K+}$ gravimetrically. Old-timers may remember the feared Kalignost. $\ce{XBPh4-}$, for X=$\ce{Rb+, Cs+, NH4+,Tl+}$ is similarly insoluble.
Thanksfully, now there is methods like AAS, and we plague the kids with that in Instrumental Analysis/Analytical Chemistry classes instead.
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Perhaps the simplest case involving limited (<0.1 molar) solubility is lithium fluoride, whose solubility is only about one part in 750 by mass at 25°C (about 0.05 molar).
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There are some cations whose Group I/ammonium salts are not soluble in water. For example, (thanks Nicolau) the diuranate of ammonium is insoluble in water.
Additionally, (as I just found) the hydrides (H-) of alkali metals are not soluble, it seems, in any room-temperature liquid solvent. They hydrolyze violently (http://goo.gl/Dl8Bd4), and the hydride ion has never been observed in solution.
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3$\begingroup$ I'm not sure whether it's right to say that substances that undergo solvolysis aren't soluble. Technically, they do dissolve, they just react immediately afterwards. $\endgroup$ – Nicolau Saker Neto Feb 22 '14 at 23:34
