What would the concentration of CH3COO be at pH 5.3 if 0.1M CH3COOH was adjusted to that pH. Quiz No. 3What would the concentration of CH3C00 be at pH 5.3 if 0.1MCH3C00H was adjusted to that pH1) pH = pK + Log [A ]%3D[HA]2) CH3C00H CH3C00 +H3) Find equilibrium value of [A ]i.e [CH3C00 ]4) pH = 5.3; pK = 4.765) Let X = amount of CH3COOH dissociated at equilibrium[A ] = [X][HA] = [0.1 - X]6) 5.3 = 4.76 + Log [XI[0.1- X]

Henderson-Hasselbach equation. this equation shows the relationship between pH of a solution, the…

Answered: What would the concentration of CH3C00…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.17QAP

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Calculate the pH of a weak acid which dissociates as AH ⇌ A- + H+ ( like CH3COOH ⇌ CH3COO- + H+ or HNO2 ⇌ NO2- + H+ ) knowing that the initial concentrations are [AH]0 0.11 M and the acid dissociation constant, Ka , is 5.86e-7 pH _______ ← please insert your value
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please help me answer all 4 a. In the laboratory a student measures the percent ionization of a 0.537 M solution of formic acid , HCOOH to be 1.89 %. Calculate value of Ka =_______ from this experimental data. b. Calculate the percent ionization of a 0.580 M solution of hypochlorous acid. % Ionization = _______ c. In the laboratory, a general chemistry student measured the pH of a 0.537 M aqueous solution of trimethylamine, (CH3)3N to be 11.781. Use the information she obtained to determine the Kb for this base. Kb(experiment) =____________ d. In the laboratory, a general chemistry student measured the pH of a 0.586 M aqueous solution of triethanolamine, C6H15O3N to be 10.780. Use the information she obtained to determine the Kb for this base. Kb(experiment) = ________________
a) If the pH value of an aqueous solution of trimethylamine [(CH3)3N] is 10.75, what should be the molarity of this solution? (CH3)3N + H2O ↔ (CH3)3NH+ + OH-, Kb = 6,3 × 10-5 b) What will be the pH of the solution prepared by dissolving 8.35 g of aniline hydrochloride (C6H5NH3+Cl-) in 750 mL of 0.215 M aniline (C6H5NH2)? Is this solution an effective buffer? Explain (Kb = 7,4 × 10-10 for aniline, C: 12.0 g / mol, H: 1.0 g / mol, N: 14.0 g / mol, Cl: 35.4 g / mol) .
a) If the pH value of an aqueous solution of trimethylamine [(CH3) 3N] is 10.75, what should be the molarity of this solution? (CH3) 3N + H2O ↔ (CH3) 3NH + + OH-, Kb = 6.3 × 10-5 b) What will be the pH of the solution prepared by dissolving 8.35 g of aniline hydrochloride (C6H5NH3 + Cl-) in 750 mL of 0.215 M aniline (C6H5NH2)? Is this solution an effective buffer? Explain (Kb = 7.4 × 10-10 for aniline, C: 12.0 g / mol, H: 1.0 g / mol, N: 14.0 g / mol, Cl: 35.4 g / mol) .
A.) Calculate the pH of a 0.359 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4) and the equilibrium concentrations of the weak acid and its conjugate base.plz include all three pH, [HF]M,[F-]M the last person didn't do it so having to waste a second question pH = [HF ]equilibrium = M [F- ]equilibrium = M B.) Calculate the pH of a 0.0230 M aqueous solution of acetylsalicylic acid (HC9H7O4, Ka = 3.4×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. plz include all three parts of the answer the last person didn't do it so having to waste a second question pH = [HC9H7O4]equilibrium = M [C9H7O4- ]equilibrium = M

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