Caffeine is about 10 times as soluble in hot water as in cold water. a chemist puts a hot-water extract of caffeine into an ice bath, and some caffeine crystallizes. is the remaining solution saturated, unsaturated, or supersaturated and why?

Supersaturated solution

Explanation:

A super-saturated solution is on that contains more than the amount of solute needed to saturate it at a particular temperature.

In our problem, Caffeine solution was saturated when it was in hot water because it was at a temperature where the solubility is high. Immediately it was introduced to an ice bath, a new temperature is recorded. At that lower temperature only a very less amount of caffeine is needed to saturate the solution, hence the excess crystallizes out and makes the solution super-saturated

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"