A chemist must prepare 550.0 mL of nitric acid solution with a pH of 1.90 at 25 °C. He will do this in three steps: • Fill a 550.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (7.0M) stock nitric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated nitric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. mL

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A chemist must prepare 550.0 mL of nitric acid solution with a pH of 1.90 at 25 °C.
He will do this in three steps:
• Fill a 550.0 mL volumetric flask about halfway with distilled water.
• Measure out a small volume of concentrated (7.0M) stock nitric acid solution and add it to the flask.
• Fill the flask to the mark with distilled water.
Calculate the volume of concentrated nitric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits.
mL
Transcribed Image Text:A chemist must prepare 550.0 mL of nitric acid solution with a pH of 1.90 at 25 °C. He will do this in three steps: • Fill a 550.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (7.0M) stock nitric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated nitric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. mL
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