Sure you can! (at least with SnCl2, stored over CaCl2 at room temp for several days...)
And why use a solvent at all? Molecular sieves work fine for drying gases; and all drying processes rely on the fact that crystal water is always given off as soon as the drying agent's hydrate bond represents a less energy-consuming type of bonding compared to the substrate, meaning that the drying agent has a greater affinity for water than the substance to be dried, either alone or with the help of vacuum and/or heat (which both make it harder for the water to stay in the crystal lattice, therefore it leaves at some point..). Bonus: ions have a hard time wandering through air, not to speak of vacuum. I doubt that any reaction between the drying agent and compound to be dried can take place in a dessicator.
Mol sieves further work a lot better if heated, so I don't see why you would want to expose any ergot compound to the possible danger of destruction, just to be able to dry it together with some solvent... ::)
Maybe I should've asked "why in any way should a solvent be better in terms of transporting the water to the sieves, compared to plain air having a pressure of <1 atm?"
it all depends on the thermal gravimetry peak:
Post 506649 (https://www.thevespiary.org/talk/index.php?topic=10548.msg50664900#msg50664900)
(Rhodium: "drying ammonium acetate", Newbee Forum)
Post 71294 (missing)
(lugh: "Re: Anhydrous or not....", Methods Discourse)
Post 442008 (https://www.thevespiary.org/talk/index.php?topic=6557.msg44200800#msg44200800)
(L_jamf: "ammonium acetate preparation", Chemistry Discourse)
indole_amine