Please answer the question all information is provided Data and Calculations1. Measurement of pH and titration of acetic acid solutionConcentration of standardized NaOH titrant 0. 1029mol/LMass concentration of acetic acid2.40g/LTrial 1Trial 2Trial 3Measured pH of the acetic acid solution3.103.123.1230.0830.0430.05Mass of acetic acid solution taken for titrationgggInitial buret reading of NaOH titrant2.3014.025.737.311.61.191.190.0396 mol/L60.61 g/molmLmLmL14.0I1.71.20Final buret reading of NaOH titrant25.711.7mLmLmLNet volume of NaOHFinnl-initolmLmLmLMillimoles of NaOH to end point of titrationmmol1.20mmolmmolMillimoles of acetic acid in sample1.20 mmol|.20mmolmmol0.040 mol/L60.16 8/molMolar concentration of acetic acid solution0.040mol/LCalculated molar mass of acetic acid(0.08 8/molCalculation of the ionization constant for acetic acid from the measured pH of the acetic acidsamples. (Average the pH and molar concentration values for the samples of acetic acid you titrated; use theaverage values in the calculation of the ionization constant.)60.28Average molar concentration of acetic acid for the samples you titrated:mol/L3.1Average pHCalculate the corresponding [H3O*], compute the concentration of A¯ and HA, and calculate the dissociationconstant, K,.M H3O+M AМ НА[H;O*][A]KaНА)pk, =

Calculation of the ionization constant for acetic acid from the measured pH of the acetic acid samples. (Average the pH and molar concentration values for the samples of acetic acid you titrated; use the average values in the calculation of the ionization constant.) 60.28 Average molar concentration of acetic acid for the samples you titrated: mol/L 3.11 Average pH Calculate the corresponding [H3O*], compute the concentration of A and HA, and calculate the dissociation constant, Ką. M H30* МА- М НА [H;O*][A] K. НА pK,

Calculation of the ionization constant for acetic acid from the measured pH of the acetic acid samples. (Average the pH and molar concentration values for the samples of acetic acid you titrated; use the average values in the calculation of the ionization constant.) 60.28 Average molar concentration of acetic acid for the samples you titrated: mol/L 3.11 Average pH Calculate the corresponding [H3O], compute the concentration of A and HA, and calculate the dissociation constant, Ką. M H30 МА- М НА [H;O*][A] K. НА pK,

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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