A chemist must prepare 250.0 mL of nitric acid solution with a pH of 1.40 at 25 "C. He will do this in three steps: • Fill 250.0 ml volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (9.0M) 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.

Chemistry
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Chapter1: Chemical Foundations
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Question 2
A chemist must prepare 250.0 mL of nitric acid solution with a pH of 1.40 at 25 °C.
He will do this in three steps:
• Fill a 250.0 mL volumetric flask about halfway with distilled water.
• Measure out a small volume of concentrated (9.0M) 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,
O ml.
Transcribed Image Text:= Initial Knowledge Check Question 2 A chemist must prepare 250.0 mL of nitric acid solution with a pH of 1.40 at 25 °C. He will do this in three steps: • Fill a 250.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (9.0M) 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, O ml.
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