Below is the titration curve for a monoprotic weak acid/weak base. In order to produce this curv you titrate the weak acid with NaOH until its all been converted to its weak base form. Recall fro general chemistry, at 1.0 equivalents of titrant (OH-), all of your original acid analyte has been neutralized (deprotonated) and is in its basic form. Please answer the following questions. 11 10 7 6. 5 3. 2 1 0.2 0.4 0.6 0.8 1 OH Equivalents a. What is the pKa of this compound? Entry Format: Please round your answer to the nearest wh number. b. At a pH of 6 will the concentration of the conjugate base be higher or lower than the concentration of conjugate acid? Entry Format: Please type the word higher or lower with no capitalization. c. Using the pKa you calculated in part a, find the percent of molecules that are in the conjugate form at a pH of 5.2. Entry Format: Please give your answer rounded to two significant figures and do not include a percent symbol. Two sig figs looks like: 1.0 60. 19. 19 Hd

Below is the titration curve for a monoprotic weak acid/weak base. In order to produce this curv you titrate the weak acid with NaOH until its all been converted to its weak base form. Recall fro general chemistry, at 1.0 equivalents of titrant (OH-), all of your original acid analyte has been neutralized (deprotonated) and is in its basic form. Please answer the following questions. 11 10 7 6. 5 3. 2 1 0.2 0.4 0.6 0.8 1 OH Equivalents a. What is the pKa of this compound? Entry Format: Please round your answer to the nearest wh number. b. At a pH of 6 will the concentration of the conjugate base be higher or lower than the concentration of conjugate acid? Entry Format: Please type the word higher or lower with no capitalization. c. Using the pKa you calculated in part a, find the percent of molecules that are in the conjugate form at a pH of 5.2. Entry Format: Please give your answer rounded to two significant figures and do not include a percent symbol. Two sig figs looks like: 1.0 60. 19. 19 Hd

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter22: Properties Of Systems In Chemical Equilibrium-le Chatelier's Principle

Section: Chapter Questions

Problem 1ASA: Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the...

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In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
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Answer the following three questions based on the information given below. Consider a buffer made with 34.0 mL of 0.25 M butanoic acid (HC4H702) and 16.0 mL of 0.46 M sodium butanoate (NaC4H7O2). The K, for butanoic acid (HC4H-02) is 1.5 X 105. Round all numerical answers to the 100n place (2 decimal places). Assume 298 K. What is the pH, if 2.0 mL of 1.0 M NAOH is added to this buffer? Type your answer..
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This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
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This question is concerned with acid/base. The ionic product of water may be taken as 10-14 mol2dm-6. Oxalic acid (HC2CCO2H) is a dibasic acid. On the diagram below, sketch the curve showing the variation of pH when a solution of oxalic acid is neutralized with an aqueous solution of sodium hydroxide of similar concentration. The diagram should be carefully labelled.
The student Louise continued the analysis of acetic acid using half - neutralization technique. She titrates this acetic acid solution using 0.984 M NaOH titrant solution. When volume of NaOH reaches 14.34 mL, she stopped titration. The averaged pH value is measured to be 4.75. Determine the acid dissociation constant Ka.
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