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Ludmilka [50]
3 years ago
15

Calculate the volume in liters of a ×7.7310−5/mmolL silver(II) oxide solution that contains 475.μmol of silver(II) oxide AgO . R

ound your answer to
3 significant digits.
Chemistry
1 answer:
Serhud [2]3 years ago
4 0

Answer: Thus volume in liters is 6.14\times 10^3L

Explanation:

Molarity is defined as the number of moles of solute dissolved per liter of the solution.

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of silver oxide}}{\text{Volume of solution in L}}     .....(1)

Molarity of silver oxide solution = 7.73\times 10^{-5}mmol/L=7.73\times 10^{-2}\mu mol/L      1mmol=1000\mu mol

Moles of silver oxide = 475\mu mol      

Volume of solution in L = ?

Putting values in equation 1, we get:

7.73\times 10^{-2}\mu mol\L=\frac{475\mu mol}{\text{Volume of solution in L}}\\\\\{\text{Volume of solution in L}}=\frac{475\mu mol}{7.73\times 10^{-2}\mu mol\L}=6.14\times 10^3L

Thus volume in liters is 6.14\times 10^{3}L

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The two naturally occurring isotopes of antimony, 121Sb (57.21 percent) and 123Sb (42.79 percent), have masses of 120.904 and 12
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The correct answer is option c.

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