Atomic mass of Na = 22.98976928 ±0.00000033 g/mole Atomic mass of Cl = 35.4570± 0.0027 g/mole Mass of weighing paper = 1.223 ±0.003grams Mass of weighing paper + sample = 1.345 ±.007grams The sample is dissolved in water contained in a 50.00±0.02 ml volumetric flask. What is the concentration of the sample, expressed as a molarity? You should use the rules of error propagation to get your best estimate of the uncertainty in the final result, with the proper number of significant digits as well.
Atomic mass of Na = 22.98976928 ±0.00000033 g/mole Atomic mass of Cl = 35.4570± 0.0027 g/mole Mass of weighing paper = 1.223 ±0.003grams Mass of weighing paper + sample = 1.345 ±.007grams The sample is dissolved in water contained in a 50.00±0.02 ml volumetric flask. What is the concentration of the sample, expressed as a molarity? You should use the rules of error propagation to get your best estimate of the uncertainty in the final result, with the proper number of significant digits as well.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.117QE
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Transcribed Image Text:Atomic mass of Na = 22.98976928 ±0.00000033 g/mole
Atomic mass of Cl = 35.457, ± 0.0027 g/mole
%3D
Mass of weighing paper = 1.223 ±0.003grams
Mass of weighing paper + sample = 1.345 t.007grams
The sample is dissolved in water contained in a 50.00±0.02 ml volumetric flask. What is the
concentration of the sample, expressed as a molarity? You should use the rules of error
propagation to get your best estimate of the uncertainty in the final result, with the proper
number of significant digits as well.
%3D
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