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.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.

the answer is b & c i believe : )