Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW =60.05) was added to a 1 –liter volumetric flask, and the flask was filled to the mark with distilled water. A portion of the resulting solution was added to a conductance cell (k = 1.25 cm-1), and the conductance was found to be 416 μS. Calculate the dissociation constant Ka of acetic acid. ΛoH+= 349.8 Scm2/mole and ΛoCH3COO- = 41 Scm2/mole Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW =60.05) was added to a 1-litervolumetric flask, and the flask was filled to the mark with distilled water. A portion of the resultingsolution was added to a conductance cell (k = 1.25 cm³¹), and the conductance was found to be416 µS. Calculate the dissociation constant Ka of acetic acid. AºH+ = 349.8 Scm²/moleandA°CH3COO = 41 Scm²/mole

6.00 mL of acetic acid was added to a 1 L flask and filled with distilled water . A conductance…

Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW=60.05) was added to a 1-liter volumetric flask, and the flask was filled to the mark with distilled water. A portion of the resulting solution was added to a conductance cell (k = 1.25 cm¹), and the conductance was found to be 416 µS. Calculate the dissociation constant Ka of acetic acid. AºH+ = 349.8 Scm²/mole and A CH3COO = 41 Scm²/mole

Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW=60.05) was added to a 1-liter volumetric flask, and the flask was filled to the mark with distilled water. A portion of the resulting solution was added to a conductance cell (k = 1.25 cm¹), and the conductance was found to be 416 µS. Calculate the dissociation constant Ka of acetic acid. AºH+ = 349.8 Scm²/mole and A CH3COO = 41 Scm²/mole

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.8QAP

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