Why doesn't ethanol dissolve in sodium bicarbonate?

Today I experimented with different solvents and solutes and was a bit surprised by one result. When I added ethanol to dilute sodium bicarbonate and tapped the test tube against my palm to mix it, I saw the mixture swirling, then it turned cloudy.

I don't understand why this happened -- as far as my understanding goes, ethanol is both a weak acid and a weak base, and it dissolved with NaOH and HCl with no trouble. Does this have anything to with the fact that ethanol and sodium bicarbonate are both amphiprotic? Or is there a different explanation?

Thanks in advance.