Please answer this Following table indicates the readings from astandardization experiment, in which 5M phthalice:acid (2g in 200, M.Mass=166.14 g/mol) was used tostandardize the NaOH (3g in 500ml) of unknownconcentration. Calculate the concentration of NaOHusing these values.(2)Titration no.Initial VolumeFinal Volume15 ml4.2 ml24.2 ml3.5 ml33.5 ml2.6 ml

During titration, at equivalence point the number of moles of acid should be equal to number of…

Following table standardization experiment, in which 5M phthalic acid (2g in 200, M.Mass=166.14 g/mol) was used to indicates the readings from a standardize the NaOH (3g in 500ml) of unknown concentration. Calculate the concentration of NaOH using these values. (2) Titration no. Initial Volume Final Volume 1 5 ml 4.2 ml 2 4.2 ml 3.5 ml

Following table standardization experiment, in which 5M phthalic acid (2g in 200, M.Mass=166.14 g/mol) was used to indicates the readings from a standardize the NaOH (3g in 500ml) of unknown concentration. Calculate the concentration of NaOH using these values. (2) Titration no. Initial Volume Final Volume 1 5 ml 4.2 ml 2 4.2 ml 3.5 ml

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
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A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.
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,…
What volume (in mL) of 0.2968 M NaOH is required to titrate 15.00 mL of 0.2635 M HAc to the equivalence point? (give your answer to 2 decimal places)
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