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< PREV 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12 Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Kb for (CH3)3N is 5.2 × 10-4. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT A solution is prepared with 0.075 M (CH3)3N and 0.10 M (CH3)3NHCI. 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) 0 (CH3)3N(aq) + H₂O(1) OH-(aq) + (CH3)3NH+(aq) 0.075 0.10 5.2 × 10-4 +x -x RESET +2x -2x 0.075 + x 0.075 - x 0.075 + 2x 0.075 - 2x 0.10 + x 0.10 - x 0.10 + 2x 0.10 - 2x

< PREV 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12 Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Kb for (CH3)3N is 5.2 × 10-4. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT A solution is prepared with 0.075 M (CH3)3N and 0.10 M (CH3)3NHCI. 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) 0 (CH3)3N(aq) + H₂O(1) OH-(aq) + (CH3)3NH+(aq) 0.075 0.10 5.2 × 10-4 +x -x RESET +2x -2x 0.075 + x 0.075 - x 0.075 + 2x 0.075 - 2x 0.10 + x 0.10 - x 0.10 + 2x 0.10 - 2x

Chemistry
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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< PREV 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12
Transcribed Image Text:< PREV 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12
Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Kb for (CH3)3N is 5.2 × 10-4. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT A solution is prepared with 0.075 M (CH3)3N and 0.10 M (CH3)3NHCI. 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) 0 (CH3)3N(aq) + H₂O(1) OH-(aq) + (CH3)3NH+(aq) 0.075 0.10 5.2 × 10-4 +x -x RESET +2x -2x 0.075 + x 0.075 - x 0.075 + 2x 0.075 - 2x 0.10 + x 0.10 - x 0.10 + 2x 0.10 - 2x
Transcribed Image Text:Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Kb for (CH3)3N is 5.2 × 10-4. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT A solution is prepared with 0.075 M (CH3)3N and 0.10 M (CH3)3NHCI. 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) 0 (CH3)3N(aq) + H₂O(1) OH-(aq) + (CH3)3NH+(aq) 0.075 0.10 5.2 × 10-4 +x -x RESET +2x -2x 0.075 + x 0.075 - x 0.075 + 2x 0.075 - 2x 0.10 + x 0.10 - x 0.10 + 2x 0.10 - 2x
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