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If the pH of a solution is 2.78 with an absolute uncertainty of ±0.05, what is the [H+] and its uncertainty? O [H*] = 1.66 x 10³ M uncertainty in the concentration= O [H] = 1.66 x 10-³ M uncertainty in the concentration 1.91 x 10- M O [H+] = 1.34 x 10-4 M uncertainty in the concentration= 1.78 x 105 M O [H] 1.25 x 10-5 M B 1.33 x 10 M uncertainty in the concentration 1.65 x 10-5 M

If the pH of a solution is 2.78 with an absolute uncertainty of ±0.05, what is the [H+] and its uncertainty? O [H*] = 1.66 x 10³ M uncertainty in the concentration= O [H] = 1.66 x 10-³ M uncertainty in the concentration 1.91 x 10- M O [H+] = 1.34 x 10-4 M uncertainty in the concentration= 1.78 x 105 M O [H] 1.25 x 10-5 M B 1.33 x 10 M uncertainty in the concentration 1.65 x 10-5 M

Chemistry: Principles and Practice
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
Chapter15: Solutions Of Acids And Bases
Section: Chapter Questions
Problem 15.54QE: Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+,...
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If the pH of a solution is 2.78 with an absolute uncertainty of ±0.05, what is the [H+] and its uncertainty? O [H+] = 1.66 x 10-3 M uncertainty in the concentration O [H+] = 1.66 x 10-3 M uncertainty in the concentration O [H+] = 1.34 x 10-4 M uncertainty in the concentration 1.78 x 10-5 M O [H+] 1.33 x 10 M -4 uncertainty in the concentration= 1.91 x 10-4 M -1.25 x 10-5 M 1.65 x 10-5 M
Transcribed Image Text:If the pH of a solution is 2.78 with an absolute uncertainty of ±0.05, what is the [H+] and its uncertainty? O [H+] = 1.66 x 10-3 M uncertainty in the concentration O [H+] = 1.66 x 10-3 M uncertainty in the concentration O [H+] = 1.34 x 10-4 M uncertainty in the concentration 1.78 x 10-5 M O [H+] 1.33 x 10 M -4 uncertainty in the concentration= 1.91 x 10-4 M -1.25 x 10-5 M 1.65 x 10-5 M
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