Please help with A, B, C, D, and E CH3COOH (I) + H₂O (1)→ H₂O* (aq) + CH3COO (aq)K. (acetic acid) =A) The Ka for acetic acid is 1.8X105. If the initial concentration of acetic acid is 0.012 M. Calculatethe [H₂O*] coming ONLY from acetic acid using an ice table. Show all steps of calculation.Reaction stage[CH₂COOH] (M)[CH3COO] (M)[H₂O¹] (M)0Initial0.012ChangeEquilibriumK. (acetic acid) = 1.8x10-5[H3O+] =0B) On question 1B you calculated the [H3O+] coming only from autoproteolysis of water. That valueis-110°. How does this number compare with the [H3O+] coming only from aceticacid as calculated above?C) Calculate pH of this 0.012 M acetic acid in water considering the hydronium generated from theacid as well as the solvent. Where pH = -log[H3O*].D) Calculate pH of the solution containing 0.012 M acetic acid in water considering the hydroniumgenerated ONLY from the acid. Where pH = -log[H3O+].E) Most common pH meters can only read two decimal places. Based on this information, would youfor all practical purpose consider the hydronium concentration coming from water whenconsidering pH of a strong acid? Explain.3

Given: An acid acid solution with initial concentration is 0.012 M.To find: [H3O+] coming from…

A) The Ka for acetic acid is 1.8X105. If the initial concentration of acetic acid is 0.012 M. Calculate the [H₂O*] coming ONLY from acetic acid using an ice table. Show all steps of calculation. Reaction stage [CH₂COOH] (M) [CH3COO] (M) [H₂O¹] (M) 0 0.012 Initial Change Equilibrium K. (acetic acid) = 1.8x10-5 [H₂O*] = 0 B) On question 1B you calculated the [H3O+] coming only from autoproteolysis of water. That value is . How does this number compare with the [H3O+] coming only from acetic acid as calculated above? 10-7 C) Calculate pH of this 0.012 M acetic acid in water considering the hydronium generated from the acid as well as the solvent. Where pH = -log[H3O*]. D) Calculate pH of the solution containing 0.012 M acetic acid in water considering the hydronium generated ONLY from the acid. Where pH = -log[H3O*]. E) Most common pH meters can only read two decimal places. Based on this information, would you for all practical purpose consider the hydronium concentration coming from water when considering pH of a strong acid? Explain.

A) The Ka for acetic acid is 1.8X105. If the initial concentration of acetic acid is 0.012 M. Calculate the [H₂O] coming ONLY from acetic acid using an ice table. Show all steps of calculation. Reaction stage [CH₂COOH] (M) [CH3COO] (M) [H₂O¹] (M) 0 0.012 Initial Change Equilibrium K. (acetic acid) = 1.8x10-5 [H₂O] = 0 B) On question 1B you calculated the [H3O+] coming only from autoproteolysis of water. That value is . How does this number compare with the [H3O+] coming only from acetic acid as calculated above? 10-7 C) Calculate pH of this 0.012 M acetic acid in water considering the hydronium generated from the acid as well as the solvent. Where pH = -log[H3O]. D) Calculate pH of the solution containing 0.012 M acetic acid in water considering the hydronium generated ONLY from the acid. Where pH = -log[H3O]. E) Most common pH meters can only read two decimal places. Based on this information, would you for all practical purpose consider the hydronium concentration coming from water when considering pH of a strong acid? Explain.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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