Question

a chemistry student is given 3.00 l of a clear aqueous solution at 30.°c. he is told an unknown amount of a certain compound x is dissolved in the solution. the student allows the solution to cool to 30.°c. the solution remains clear. he then evaporates all of the water under vacuum. a precipitate remains. the student washes, dries and weighs the precipitate. it weighs 0.72 kg. using only the information above, can you calculate the solubility of x in water at 30.°c? if you said yes, calculate it. be sure your answer has a unit symbol and the right number of significant digits. yes no

Explanation:

Step1: Determine the mass of the compound

The mass of the precipitate is \(0.72\space kg\). But we need to find the solubility. Solubility is defined as the mass of solute per \(100\space g\) (or \(0.1\space kg\)) of solvent. However, we are not given the mass of water (the solvent) in the original solution.

Step2: Analyze the given information

We know the volume of the solution (\(3.00\space L\)), but without knowing the density of the solution (to convert volume to mass) or the mass of water (solvent) in the solution, we cannot calculate the solubility (which is mass of solute per mass of solvent).

Answer:

no