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Alex_Xolod [135]
3 years ago
9

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.
Chemistry
1 answer:
kenny6666 [7]3 years ago
8 0

The student made a mistake because he did not convert a unit of volume from milliliters to liters. After all, molarity is defined as the number of moles of solute per liter of solution.

Answer: C=0.406M.C=0.406M.

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Answer:

4

Explanation:

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Avogadro constant:-

N_a=6.023\times 10^{23}

Hence,

Mass of XeF_n = 131.293+ n18.998 g

So,

6.023\times 10^{23}  molecules have a mass of 131.293+ n18.998 g

Also,

1  molecules have a mass of \frac{(131.293+ n18.998)}{6.023\times 10^{23}} g

So,

5.0\times 10^{20}  molecules have a mass of \frac{(131.293+ n18.998)}{6.023\times 10^{23}}\times 5.0\times 10^{20} g

Also, given mass = 0.172 g

Thus,

\frac{(131.293+ n18.998)}{6.023\times 10^{23}}\times 5.0\times 10^{20}=0.172

\frac{18.998n+131.293}{1204.6}=0.172

18.998n+131.293=207.1912

n=\frac{75.8982}{18.998}=4

<u>Thus, value of n is 4.</u>

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