Determine the concentration of C6H5NH3 in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of C6H5NH3+. The Kb for C6H5NH2 is 3.8 x 10-10. Complete Parts 1-3 before submitting your answer. 2 NEXT > A buffer solution contains dissolved C6H5NH2 and C6H5NH3Cl. The initial concentration of C6H5NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of C6H5NH3+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) C6H5NH2(aq) H₂O(1) 14 OH(aq) C6H5NH3+(aq) RESET 0 0.50 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 x 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x+6.3 x 10-5 x-6.3 x 10-5 x+1.6 × 10-10 x-1.6 × 10-10 x+3.8 × 10-10 x-3.8 × 10-10 MacBook Air Determine the concentration of C6H5NH3 in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of C6H5NH3+. The Kb for C6H5NH2 is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3. [C6H5NH3] = M RESET 0 8.3 x 1010 0.86 1.2 10 2.1 0.50
Determine the concentration of C6H5NH3 in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of C6H5NH3+. The Kb for C6H5NH2 is 3.8 x 10-10. Complete Parts 1-3 before submitting your answer. 2 NEXT > A buffer solution contains dissolved C6H5NH2 and C6H5NH3Cl. The initial concentration of C6H5NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of C6H5NH3+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) C6H5NH2(aq) H₂O(1) 14 OH(aq) C6H5NH3+(aq) RESET 0 0.50 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 x 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x+6.3 x 10-5 x-6.3 x 10-5 x+1.6 × 10-10 x-1.6 × 10-10 x+3.8 × 10-10 x-3.8 × 10-10 MacBook Air Determine the concentration of C6H5NH3 in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of C6H5NH3+. The Kb for C6H5NH2 is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3. [C6H5NH3] = M RESET 0 8.3 x 1010 0.86 1.2 10 2.1 0.50
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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Can you please set up the ice table?
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