please all blank questions on all 3 pictures thank you!! A 50.00-ml sample of a 0.250 M solution of butyric acid, HB, (K, = 1.5 x 105) is titrated with 0.125 M NaOH.%3!Complete the following tables to calculate the equilibrium [H'] and pH of the initial solution.Set up: Do not use spaces.[HB][B'][H*]Initial concentration0.250Expression for change in concentration (-x, +x, -2x, +2x, etc)-X++Expression for equilbrium concentration (see above instruction)0.250-xNumerical answers:[HB][B'][H']nitial concentration, mol/L0.25040Change in concentration, mol/LEquilibrium concentration, mol/LpH= Numerical answers:[B'][HB)[OH']Initial concentration, mol/LChange in concentration, moLEquilibrium concentration, mol/L[H*] =mol/LpH =Calculatethe number of moles of butyric present in the initial solution:mol- the volume of NaOH solution needed to reach equivalence point:mL- the total volume of the titration mixture:ml.- the initial concentration of the conjugate base of butyric acid, B", in the titrated mixture:mol/L- Ko of the conjugate base of butyric acid:- pH halfway to the equivalence point:Complete the following tables to calculate the equilibrium [H*] and pH of the titrated solution.Set up: Do not use spaces.[B'][HB')[OH']Initial concentrationExpression for change in concentration (-x, +x, -2x, +2x, etc)Expression for equilibrium concentration (see above instruction)Numerical answers:this is a chemistry question

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A 50.00-mL sample of a 0.250 M solution of butyric acid, HB, (K = 1.5 x 10 ) is titrated with 0.125 M NaOH. Complete the following tables to calculate the equilibrium [H'] and pH of the initial solution. Set up: Do not use spaces. (HB) [B'] [H'] Initial concentration 0.250 Expression for change in concentration (-x, +x, -2x, +2x, etc) ++ Expression for equilibrium concentration (see above instruction) 0.250-x Numerical answers: (HB) (B] [H'] nitial concentration, mol/L 0.250 Change in concentration, mol/L Equilibrium concentration, mol/l pH =

A 50.00-mL sample of a 0.250 M solution of butyric acid, HB, (K = 1.5 x 10 ) is titrated with 0.125 M NaOH. Complete the following tables to calculate the equilibrium [H'] and pH of the initial solution. Set up: Do not use spaces. (HB) [B'] [H'] Initial concentration 0.250 Expression for change in concentration (-x, +x, -2x, +2x, etc) ++ Expression for equilibrium concentration (see above instruction) 0.250-x Numerical answers: (HB) (B] [H'] nitial concentration, mol/L 0.250 Change in concentration, mol/L Equilibrium concentration, mol/l pH =

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 57P

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