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iren [92.7K]
3 years ago
14

A chemist adds 135.0 mL of a 0.21M zinc nitrate (Zn(NO3) solution to a reaction flask. Calculate the mass in grams of zinc nitra

te the chemist has added to the flask. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
yKpoI14uk [10]3 years ago
8 0

Answer:

5.36 grams the mass in grams of zinc nitrate the chemist has added to the flask.

Explanation:

Molarity=\frac{\text{Moles of solute}}{\text{Volume of the solution (L)}}

Moles of zinc nitrate = n

Volume of the solution = 135.0 mL = 0.1350 L

Molarity of the solution = 0.21 M

0.21 M=\frac{n}{0.1350 L}

n=0.21M\times 0.1350 L=0.02835 mol

Mass of 0.02835 moles of zinc nitrate:

0.02835 mol × 189 g/mol = 5.358 g ≈ 5.36 g

5.36 grams the mass in grams of zinc nitrate the chemist has added to the flask.

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