During the extraction lab expirement, how does anhydrous sodium sulfate \"dries\
ID: 489171 • Letter: D
Question
During the extraction lab expirement, how does anhydrous sodium sulfate "dries" the methylene chloride solution? Use chemical properties to explain your answer.
Context: During lab we had this Methylene chloride solution we extracted using a seperatory flask. The organic layer which was made of this methlene chloride solution was "dried" using anhydrous sodium sulfate. The sulfate started to clump up at the bottom until the added sulfate would not clump and be free flowing. I realize that the Sulfate soaks up all the water, but Im not sure why chemically. Thanks!
Explanation / Answer
Sodium sulfate is an important compound of sodium. When anhydrous, it is a white crystalline solid of formula Na2SO4. The decahydrate, Na2SO4 .Sodium sulfate is chemically very stable - it does not decompose, even if heated, and it does not react with oxidizing or reducing agents at normal temperatures. 10H2O, is known as Glauber's salt .Crystals sodium sulphate consist of [Na(OH2)6]+ ions with octahedral molecular geometry. These octahedral share edges such that eight of the 10 water molecules are bound to sodium and two others are interstitial, being hydrogen bonded to sulfate. These cations are linked to the sulfate anions via hydrogen bonds. Crystalline sodium sulfate decahydrate is also unusual among hydrated salts in having a measureable residual entropy (entropy at absolute zero) of 6.32 J·K1·mol1. This is ascribed to its ability to distribute water much more rapidly compared to most hydrates. As we add sodium sulphate unhydrate it tend to absorb water to form into octahedral complex.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.