Using the information from the previous question, answer the following questions(Note, use the E format for very small values, eg 1.0E-5 instead of 1.0x10-5)d. What is the Ka for this reaction?You can note any calculations you use heree. Using the approximation method, calculate the concentration of H3O+You can note any calculations you use heref. Calculate the pH of the solutionYou can note any calculations you use here The pka of ethanoic acid, (CH3COOH) (0.1 M), is 2.6 at 25°C.Write the balanced chemical equation for the ionisation of CH3COOH.a.b.C.Ka =Write the expression for the equilibrium constant, KaComplete the initial-change-equilibrium table for the species in the reactionConc (mol L-1) CH³COOH CH³COO¯ H³O+Initial0.100ChangeEquilibriumCH3COOH+H3O+0.1-x +XCH3COO-0OH-[CH3COOH] [CH3COO-]+0.2 -0.1 -XH3O+H₂OH₂O

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The pka of ethanoic acid, (CH3COOH) (0.1 M), is 2.6 at 25°C. Write the balanced chemical equation for the ionisation of CH3COOH. a. b. C. Ka = Write the expression for the equilibrium constant, Ka 0.1-x Conc (mol L-1) CH3COOH CH3COO- H3O+ Initial 0.100 Change BB Equilibrium + Complete the initial-change-equilibrium table for the species in the reaction CH3COOH CH3COO- H3O+ +X 0 OH- [CH3COOH] [CH3COO-] + 0.2 -0.1 -X H3O+ H₂O H₂O

The pka of ethanoic acid, (CH3COOH) (0.1 M), is 2.6 at 25°C. Write the balanced chemical equation for the ionisation of CH3COOH. a. b. C. Ka = Write the expression for the equilibrium constant, Ka 0.1-x Conc (mol L-1) CH3COOH CH3COO- H3O+ Initial 0.100 Change BB Equilibrium + Complete the initial-change-equilibrium table for the species in the reaction CH3COOH CH3COO- H3O+ +X 0 OH- [CH3COOH] [CH3COO-] + 0.2 -0.1 -X H3O+ H₂O H₂O

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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