According to Example 14-1, the mass percent ethanol in a particular aqueous solution is less than the volume percent in the same solution. Explain why this is also true for all aqueous solutions of ethanol. Would it be true of all ethanol solutions, regardless of the other component? Explain.

Example 14-1

An ethanol–water solution is prepared by dissolving 10.00 mL of ethanol, CH₃CH₂OH (d = 0.789 g/mL), in a sufficient volume of water to produce 100.0 mL of a solution with a density of 0.982 g/mL(Fig. 14-1). What is the concentration of ethanol in this solution expressed as 

(a) Volume percent; 

(b) Mass percent; 

(c) Mass/volume percent; 

(d) Mole fraction; 

(e) Mole percent;

(f) Molarity; 

(g) Molality?

Figure 14-1

Transcribed Image Text:

Water 10.00 mL CH3CH₂OH Volumetric flask 100.0 mL→ Ethanol-water solution: d = 0.982 g/mL