@ Prepare a "pH curve" as follows:a) Find the pH of the acid solution just before the end pointwhen 0.1 ml of base less than the end point voiume has beenadded.potnt, therefore at the end of the titration ph - 7.We are assuming that end point equals equivalenceb) Repeat calculation 'a' for a volume 1 ml less and 5 ml lessthen end point and before any base is added. That is Oml base added.)Before end point, we assume that all the base is used up bythe acid.c) Assuming you had continued the titration past the end point,calculate the pH when 0.1 ml of base beyond end point hadbeen added.d) Repeat calculation 'c' for 1 ml, S ml and 10 ml of base beyondend point.Show all calculations and record your results in a tablesimilar ta the one shown below:excess H+excess OH0 -5 -1ENDPT-.1+.1+1+5+10(ML)BASE VOLUME20 24 24-9 25 25.1|26 30 35pH

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@ Prepare a "pH curve" as follows: a) Find the pH of the acid solution just before the end point when 0.1 ml of base less than the end point voiume has been added. potnt, therefore at the end of the titration ph = 7. We are assuming that end point equals equivalence b) Repeat calculation 'a' for a volume 1 ml less and 5 ml less then end point and before any base is added.(TThat is Oml base added. I Before end potnt, we assume that all the base is used up by the acid. c) Assuming you had continued the titration past the end point, calculate the pH when 0.1 ml of base beyond end point had been added. d) Repeat calculation 'c' for 1 ml, S ml and 10 ml of base beyond end point. Show all calculations and record your results in a table similar to the one shown below: excess H+ excess OH END 0 -5 -1 +5 +10 -.1 PT +.1 +1 (ML) BASE VOLUME O 20 24 24-9 25 25.26 30| 35 _pH

@ Prepare a "pH curve" as follows: a) Find the pH of the acid solution just before the end point when 0.1 ml of base less than the end point voiume has been added. potnt, therefore at the end of the titration ph = 7. We are assuming that end point equals equivalence b) Repeat calculation 'a' for a volume 1 ml less and 5 ml less then end point and before any base is added.(TThat is Oml base added. I Before end potnt, we assume that all the base is used up by the acid. c) Assuming you had continued the titration past the end point, calculate the pH when 0.1 ml of base beyond end point had been added. d) Repeat calculation 'c' for 1 ml, S ml and 10 ml of base beyond end point. Show all calculations and record your results in a table similar to the one shown below: excess H+ excess OH END 0 -5 -1 +5 +10 -.1 PT +.1 +1 (ML) BASE VOLUME O 20 24 24-9 25 25.26 30| 35 _pH

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 132IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...

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A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
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20 ml. of 0.5 N CH3COOH is diluted with water to 100 ml. the resulted solution is titreted with 0.5N NaOH . Calculate the pH, 1-a-atthestart b-when8ml,10ml,and15mlofNaOHhasbeen adding. C- at the equivalent point d- when 30 ml, 35 ml, 40 ml of NaOH has been Added. 2- Show the general form of the titration carve? (Ka=1.86*10-5)