Why are hydrogen-bonded compounds (such as NH3) excellent solvents for most lab reagents? [closed]

Hydrogen bonds are said to be one of the strongest molecular interactions in nature. Then why can most substances that interact through hydrogen bondig such as water and $$\ce{NH3}$$ able to dissolve a large variety of both ionic and covalent laboratory reagents? Does it have something to do with the structure of $$\ce{NH3}$$ or something else?

• Hydrogen bonds are the weakest interactions that still make directed bonds. Water is not "hydrogen-bonded", it makes hydrogen bonds to itself and to other substances, in 99% of the cases these are exactly those substances that mix well with or are soluble in water. – Karl Jan 18 '19 at 16:46
• Who says they're "excellent"? Most compounds aren't particularly soluble in them or react. – Mithoron Jan 18 '19 at 21:02
• @Mithoron Thank you for the point. On research, found that most existing compounds (by numbers) aren't soluble in solvents that interact through hydrogen-bonding. Edited the question to "laboratory reagents" from "compounds". – Kartik Jan 20 '19 at 4:24

Thus, anions and electronegative atoms in polarized molecules have very strong electrostatic interactions with the low-electron-density hydrogen atom in $$\ce{NH3}$$ or $$\ce{H2O}$$, for example. Cations and positively charged elements in polarized molecules can also be stabilized by the electronegative atoms in molecules exhibiting hydrogen bonding ($$\ce{N}$$ and $$\ce{O}$$ in this case).
These strong interparticular interactions ultimately result in polarized or ionic solutes generally being very soluble in solvents with hydrogen bonding such as $$\ce{NH3}$$ or $$\ce{H2O}$$.