A student calculated the molarity of a solution prepared by dissolving 0.730 mol of table sugar (sucrose, C12H22O11) in 1.8×10^3 m

Question

A student calculated the molarity of a solution prepared by dissolving 0.730 mol of table sugar (sucrose, C12H22O11) in 1.8×10^3 mL of water as 4.06×10^-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.

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.
please help!

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Peyton 11 months 2021-06-30T15:37:28+00:00 1 Answers 0 views 0

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    2021-06-30T15:38:53+00:00

    Answer:

    198.56 how are you doing today

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