Answered: What is the pH of 0.010 M HCl (aq)…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 4CO

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in the titration of 50.0 mL of 0.0200 M C6H5COOH(aq) with 0.100 M NaOH(aq), what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?
A 20.00 mL aliquot of sorbic acid solution (HC6H7O2) was titrated with 0.0985 M NaOH * (aq) using both an indicator and a pH meter. Ka (HC6H7O2) , is 1.7*10^ -5 . A total of 25.34 mL of 0.0985 M NaOH * (aq) was required to reach the equivalence point a) Calculate the molarity of the sorbic acid solution. b) Calculate the pH of the sorbic acid solution (use the RICE table) . c) .Calculate the pH and [C6H 7 O 2-] at the half-equivalence point . d) Calculate the pH at the equivalence point of the titration . (use Kb for hydrolysis of sorbate anion and RICE table ). e)Suggest an appropriate indicator for titration . Explain your choice . f) Calculate the pH of the solution after 10.00 mL of 0.0985 M NaOH * (aq) was added . (find moles of sorbic acid and sorbate and use Henderson Haselbalch equation ) Indicator pKa Phenolphthalein 9.3 Bromothymol blue 7.0 Methyl red. 5.0 Thymol blue. 2.0 Methyl violet…
What is the pH of 0.018M C5H5N(aq)?
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Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?

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What is the pH of 0.010 M HCl (aq) using activity coefficients?