Molar Mass of Potassium Phosphate (K3PO4): 212.27 g/mol
Density of Water: 1.00 kg/L
Solutions of known concentration can be prepared either by dissolving a known mass of solute in a solvent and diluting to a desired final volume or by diluting the appropriate volume of a more concentrated solution (a stock solution) to the desired final volume.
The solution prepared by Jennifer:
An experiment in chm 2045 requires students to prepare a 1.0 m aqueous solution of potassium phosphate.
Jennifer fills a 1.0 liter volumetric flask to the calibration line with water. She then weighs out 212.3 g of potassium phosphate and adds it to the volumetric flask.
Joe weighs out 212.3 g of potassium phosphate and adds it to a 1.0 liter volumetric flask. He then fills the volumetric flask to the calibration line with water.
Which student has correctly prepared a 1.0 m aqueous solution of potassium phosphate?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Molality concept. You can view video lessons to learn Molality. Or if you need more Molality practice, you can also practice Molality practice problems.