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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 liquid water in the reaction. Before (mol) Change (mol) After (mol) H₂NNH₂(aq) H*(aq) H₂NNH₂ (aq) RESET

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 liquid water in the reaction. Before (mol) Change (mol) After (mol) H₂NNH₂(aq) H*(aq) H₂NNH₂ (aq) RESET

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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A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > A 40.0 mL of 0.200 M H₂NNH₂ was titrated with 10.0 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE 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 liquid water in the reaction. Before (mol) Change (mol) After (mol) 6.00 x 10 Initial (M) Change (M) Equilibrium (M) -X 0.140-x 0 -6.00 x 10³ 0 1 1 0.200 + x H₂NNH₂(aq) 0.200 0.175 + x 7.00 x 10³ H₂NNH₂(aq) + 2 0.200 0.200 - x 0.175-x 0.100 2 -7.00 x 10" A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 3 Upon completion of the acid-base reaction, the H₂NNH3* ion is in equilibrium with water. Set up the ICE table in order to determine the unknown concentrations of reactants and products.. + 0.0200 H₂O(l) 0.0200 + x 3 1.00 x 10" 8.00 × 10³ 0.100 H*(aq) 0.0200 - x -1.00 x 10" -8.00 × 10³ 4 OH(aq) 0.140 2.00 x 10 0.100 + x 4 H₂NNH3 + (aq) 0.175 RESET -2.00 x 10" 0.100 - x + H₂NNH3*(aq) NEXT RESET +x 0.140 + x
Transcribed Image Text:A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > A 40.0 mL of 0.200 M H₂NNH₂ was titrated with 10.0 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE 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 liquid water in the reaction. Before (mol) Change (mol) After (mol) 6.00 x 10 Initial (M) Change (M) Equilibrium (M) -X 0.140-x 0 -6.00 x 10³ 0 1 1 0.200 + x H₂NNH₂(aq) 0.200 0.175 + x 7.00 x 10³ H₂NNH₂(aq) + 2 0.200 0.200 - x 0.175-x 0.100 2 -7.00 x 10" A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 3 Upon completion of the acid-base reaction, the H₂NNH3* ion is in equilibrium with water. Set up the ICE table in order to determine the unknown concentrations of reactants and products.. + 0.0200 H₂O(l) 0.0200 + x 3 1.00 x 10" 8.00 × 10³ 0.100 H*(aq) 0.0200 - x -1.00 x 10" -8.00 × 10³ 4 OH(aq) 0.140 2.00 x 10 0.100 + x 4 H₂NNH3 + (aq) 0.175 RESET -2.00 x 10" 0.100 - x + H₂NNH3*(aq) NEXT RESET +x 0.140 + x
A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 1 2 3 NEXT > The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0.200 + x] [0] [0.175 + x] 0 [0.200] 1.70 [0.200 -x] [0.175-x] Kb = 1 4.77 x 10-1⁰ 12.3 [0.0200] [0.0200 + x] [0.0200 -x] [0.100] 10.8 2 [0.140] [0.100 + x] 2.10 x 10-5 A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. = 3.0 x 10-6 < PREV sed on your ICE table and the equilibrium expression for Kb, determine the pH of this solution.. pH = 4.68 [0.175] 3 [0.100 -x] 4 9.32 [x] [0.140 + x] 4 RESET [2x] 3.22 [0.140 -x] RESET 0.140
Transcribed Image Text:A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 1 2 3 NEXT > The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0.200 + x] [0] [0.175 + x] 0 [0.200] 1.70 [0.200 -x] [0.175-x] Kb = 1 4.77 x 10-1⁰ 12.3 [0.0200] [0.0200 + x] [0.0200 -x] [0.100] 10.8 2 [0.140] [0.100 + x] 2.10 x 10-5 A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. = 3.0 x 10-6 < PREV sed on your ICE table and the equilibrium expression for Kb, determine the pH of this solution.. pH = 4.68 [0.175] 3 [0.100 -x] 4 9.32 [x] [0.140 + x] 4 RESET [2x] 3.22 [0.140 -x] RESET 0.140
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