Answer to Question #195813 in General Chemistry for c.c

Question #195813

A student calculated the molarity of a solution prepared by dissolving 0.730 mol of table sugar (sucrose, C12H22O11) in 1.8x10^3 mL of water as 4.06x10^-4 M C12H22O11


  • Explain the student's calculation error and explain how the student should solve for the correct value of molarity. Show a valid calculation for the molarity.


II. The student then takes a 1.00 M stock solution of table sugar (sucrose, C12H22O11) and mixes 0.305 L of stock solution with additional distilled water to create a dilute solution with a total volume of 1.25 L. 


  • Explain how the student can determine the molarity of the resulting solution. Show a valid calculation for the final molarity.
Expert's answer

1.Valid Molarity =0.347M

2.Valid final molarity =2.91M

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