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< PREV 1 2 NEXT > Based on your ICE table (Part 2) 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. Ко = = 4.3 x 10-10 RESET [0] [0.500] [0.100] [0.040] [0.700] [0.300] 闭 [2x] [0.500 + x] (0.500 - x] [0.100+x] [0.100-x] [0.040+x] (0.040-x] [0.700+x] [0.700 - x] [0.300 + x] [0.300 - x] < PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. pH = RESET 0 1.00 × 10° 1.00 × 10* 9.00 5.00 20.7 6.72 0.040 0.200 0.700 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) + CHÍNH (99) RESET 0 0.500 0.100 0.040 0.700 0.300 +x 0.500 + x 0.500-x 0.100 + x 0.100-x 0.040 + x 0.040-x 0.700 + x 0.700-x 0.300 + x 0.300-x

< PREV 1 2 NEXT > Based on your ICE table (Part 2) 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. Ко = = 4.3 x 10-10 RESET [0] [0.500] [0.100] [0.040] [0.700] [0.300] 闭 [2x] [0.500 + x] (0.500 - x] [0.100+x] [0.100-x] [0.040+x] (0.040-x] [0.700+x] [0.700 - x] [0.300 + x] [0.300 - x] < PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. pH = RESET 0 1.00 × 10° 1.00 × 10* 9.00 5.00 20.7 6.72 0.040 0.200 0.700 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) + CHÍNH (99) RESET 0 0.500 0.100 0.040 0.700 0.300 +x 0.500 + x 0.500-x 0.100 + x 0.100-x 0.040 + x 0.040-x 0.700 + x 0.700-x 0.300 + x 0.300-x

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...
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< PREV 1 2 NEXT > Based on your ICE table (Part 2) 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. Ко = = 4.3 x 10-10 RESET [0] [0.500] [0.100] [0.040] [0.700] [0.300] 闭 [2x] [0.500 + x] (0.500 - x] [0.100+x] [0.100-x] [0.040+x] (0.040-x] [0.700+x] [0.700 - x] [0.300 + x] [0.300 - x] < PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. pH = RESET 0 1.00 × 10° 1.00 × 10* 9.00 5.00 20.7 6.72 0.040 0.200 0.700
Transcribed Image Text:< PREV 1 2 NEXT > Based on your ICE table (Part 2) 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. Ко = = 4.3 x 10-10 RESET [0] [0.500] [0.100] [0.040] [0.700] [0.300] 闭 [2x] [0.500 + x] (0.500 - x] [0.100+x] [0.100-x] [0.040+x] (0.040-x] [0.700+x] [0.700 - x] [0.300 + x] [0.300 - x] < PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. pH = RESET 0 1.00 × 10° 1.00 × 10* 9.00 5.00 20.7 6.72 0.040 0.200 0.700
Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) + CHÍNH (99) RESET 0 0.500 0.100 0.040 0.700 0.300 +x 0.500 + x 0.500-x 0.100 + x 0.100-x 0.040 + x 0.040-x 0.700 + x 0.700-x 0.300 + x 0.300-x
Transcribed Image Text:Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) + CHÍNH (99) RESET 0 0.500 0.100 0.040 0.700 0.300 +x 0.500 + x 0.500-x 0.100 + x 0.100-x 0.040 + x 0.040-x 0.700 + x 0.700-x 0.300 + x 0.300-x
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