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 nitrate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

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

Explanation:

Moles of zinc nitrate = n

Volume of the solution = 135.0 mL = 0.1350 L

Molarity of the solution = 0.21 M

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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explanation:

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