NS FL9 C/P Q54

Post Reply
NS_Tutor_Thomas
Posts: 203
Joined: Wed Dec 05, 2018 6:13 pm

NS FL9 C/P Q54

Post by NS_Tutor_Thomas » Tue Jun 11, 2019 1:42 pm

A student recently wrote us: "How is BPA polar? Because in the passage it says that there was little solubility in water. So if water is polar shouldn't BPA have high solubility if it is also polar? It also say that BPA is dissolved in acetone which is nonpolar, so this made me thing BPA was a nonpolar molecule?"

Just because a molecule can form dipole-dipole intermolecular bonds does not necessarily mean that this molecule will be soluble in water. What determines whether a molecule can dissolve readily in water or not is its ability to form hydrogen bonds, which BPA cannot form. Most polar molecules can dissolve in water but BPA happens to be one that cannot. Acetone can form dipole-dipole molecular bonds because of the partial positive and negative charges on the carbonyl group. This characteristic of acetone allows for the formation of dipole-dipole bonds with BPA allowing it to dissolve in acetone. Acetone has polar and non-polar characteristics and so does BPA. Because of these properties of BPA and acetone, BPA is not classified as a nonpolar molecule.

Thanks for your question. I hope this helps!
Post Reply