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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

Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.29P: 7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its...
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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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