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< PREV 1 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ка = RESET [0] [0.95] [0.68] [8.68] [x] [2x] [2x]² [0.95+x] [0.95 - x] [0.95 + 2x] [0.95 -2x] [0.68+x] [0.68 - x] [0.68 + 2x] [0.68 - 2x] 8.68 0.939 4.79 × 10-* 2.09 × 10-º < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH RESET 0 19.65 5.46 0.95 0.022 8.53 3.4 × 10-€ 2.9 × 10-9 Press | full screen Determine the pH of a buffs 11 to exit furting an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The pKa of HBrO is 8.68. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A solution is prepared with 0.95 M HBrO and 0.68 M KBRO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HBrO(aq) + H₂O(1) = H3O+(aq) + BrO-(aq) Initial (M) Change (M) Equilibrium (M) 0 0.95 0.68 8.68 +x -x RESET +2x -2x 0.95 + x 0.95 - x 0.95 + 2x 0.95 - 2x 0.68 + x 0.68 - x 0.68 + 2x 0.68 - 2x

< PREV 1 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ка = RESET [0] [0.95] [0.68] [8.68] [x] [2x] [2x]² [0.95+x] [0.95 - x] [0.95 + 2x] [0.95 -2x] [0.68+x] [0.68 - x] [0.68 + 2x] [0.68 - 2x] 8.68 0.939 4.79 × 10-* 2.09 × 10-º < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH RESET 0 19.65 5.46 0.95 0.022 8.53 3.4 × 10-€ 2.9 × 10-9 Press | full screen Determine the pH of a buffs 11 to exit furting an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The pKa of HBrO is 8.68. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A solution is prepared with 0.95 M HBrO and 0.68 M KBRO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HBrO(aq) + H₂O(1) = H3O+(aq) + BrO-(aq) Initial (M) Change (M) Equilibrium (M) 0 0.95 0.68 8.68 +x -x RESET +2x -2x 0.95 + x 0.95 - x 0.95 + 2x 0.95 - 2x 0.68 + x 0.68 - x 0.68 + 2x 0.68 - 2x

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 103QRT: In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If...
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< PREV 1 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ка = RESET [0] [0.95] [0.68] [8.68] [x] [2x] [2x]² [0.95+x] [0.95 - x] [0.95 + 2x] [0.95 -2x] [0.68+x] [0.68 - x] [0.68 + 2x] [0.68 - 2x] 8.68 0.939 4.79 × 10-* 2.09 × 10-º < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH RESET 0 19.65 5.46 0.95 0.022 8.53 3.4 × 10-€ 2.9 × 10-9
Transcribed Image Text:< PREV 1 2 3 NEXT > Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ка = RESET [0] [0.95] [0.68] [8.68] [x] [2x] [2x]² [0.95+x] [0.95 - x] [0.95 + 2x] [0.95 -2x] [0.68+x] [0.68 - x] [0.68 + 2x] [0.68 - 2x] 8.68 0.939 4.79 × 10-* 2.09 × 10-º < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH RESET 0 19.65 5.46 0.95 0.022 8.53 3.4 × 10-€ 2.9 × 10-9
Press | full screen Determine the pH of a buffs 11 to exit furting an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The pKa of HBrO is 8.68. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A solution is prepared with 0.95 M HBrO and 0.68 M KBRO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HBrO(aq) + H₂O(1) = H3O+(aq) + BrO-(aq) Initial (M) Change (M) Equilibrium (M) 0 0.95 0.68 8.68 +x -x RESET +2x -2x 0.95 + x 0.95 - x 0.95 + 2x 0.95 - 2x 0.68 + x 0.68 - x 0.68 + 2x 0.68 - 2x
Transcribed Image Text:Press | full screen Determine the pH of a buffs 11 to exit furting an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The pKa of HBrO is 8.68. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A solution is prepared with 0.95 M HBrO and 0.68 M KBRO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HBrO(aq) + H₂O(1) = H3O+(aq) + BrO-(aq) Initial (M) Change (M) Equilibrium (M) 0 0.95 0.68 8.68 +x -x RESET +2x -2x 0.95 + x 0.95 - x 0.95 + 2x 0.95 - 2x 0.68 + x 0.68 - x 0.68 + 2x 0.68 - 2x
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