Question

The molarity of an aqueous solution of nitric acid, HNO3, is determined by titration with a 35.9 x 10^-2 M potassium hydroxide solution. If 35.9 mL of potassium hydroxide is required to neutralize 25.0 mL of the acid, what is the molarity of the nitric acid solution? Molarity = __ M

Name: the molarity of an aqueous solution of nitric acidhno3 is determined by titration with a 359 x 10 2 m potassium hydroxide solution if 359 ml of potassium hydroxide are required to neutralize 69714
Uploaded: 2022-05-28T05:32:29-08:00
Duration: 2 min 5 s
Channel: Ma Ednelyn Lim
Description: the molarity of an aqueous solution of nitric acidhno3 is determined by titration with a 359 x 10 2 m potassium hydroxide solution if 359 ml of potassium hydroxide are required to neutralize 69714

          The molarity of an aqueous solution of nitric acid, HNO3, is determined by titration with a 35.9 x 10^-2 M potassium hydroxide solution. If 35.9 mL of potassium hydroxide is required to neutralize 25.0 mL of the acid, what is the molarity of the nitric acid solution?
Molarity = __ M

Added by Jennifer K.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Ma Ednelyn Lim

05/28/2022

Step 1

Given: Molarity of potassium hydroxide solution (KOH) = 35.9 x 10^-2 M Volume of KOH used = 35.9 mL = 35.9 x 10^-3 L Moles of KOH = Molarity x Volume Moles of KOH = 35.9 x 10^-2 M x 35.9 x 10^-3 L Moles of KOH = 1.29 x 10^-3 mol Show more…

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The molarity of an aqueous solution of nitric acid, HNO3, is determined by titration with a 35.9 x 10^-2 M potassium hydroxide solution. If 35.9 mL of potassium hydroxide is required to neutralize 25.0 mL of the acid, what is the molarity of the nitric acid solution? Molarity = __ M