Find the pH of a water solution obtained by adding 1.4 mL of 1.0 M HNO2(aq) to 300.0 mL of 1.00*10^-3 M HCL(aq). The acidity constant of HNO2(aq) is 4.6*10-4 Show work and explain (Please type answer note write by hend

Find the pH of a water solution obtained by adding 1.4 mL of 1.0 M HNO2(aq) to 300.0 mL of 1.0010^-3 M HCL(aq). The acidity constant of HNO2(aq) is 4.610-4 Show work and explain (Please type answer note write by hend

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

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Question

Find the pH of a water solution obtained by adding 1.4 mL of 1.0 M HNO₂(aq) to 300.0 mL of 1.00*10^-3 M HCL(aq). The acidity constant of HNO₂(aq) is 4.6*10^-4

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Step 1: Determine number of mili mol of H+ In 300 ml of 0.001 M HCl

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Step 2: Determine number of mili mol of H+ in 1.4 ml of 1.0M HNO2

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Step 3: Determine Concentration of H+ in water solutions of HCl and HNO2

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