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A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. Before (mol) Change (mol) After (mol) 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 100 mL of 0.100 M HNO3 (a strong acid). Fill in the BCA 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.. 6.00 x 10-³ 0 1 -6.00 x 10-³ H₂NNH₂(aq) 0.100 7.00 x 10-³ 0.200 -7.00 x 10-³ + H+ (aq) 1.00 x 10-² 8.00 x 10-³ -1.00 x 10-² -8.00 x 10-³ NEXT H₂NNH3 + (aq) 2.00 x 10-³ RESET -2.00 × 10-³ +

A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. Before (mol) Change (mol) After (mol) 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 100 mL of 0.100 M HNO3 (a strong acid). Fill in the BCA 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.. 6.00 x 10-³ 0 1 -6.00 x 10-³ H₂NNH₂(aq) 0.100 7.00 x 10-³ 0.200 -7.00 x 10-³ + H+ (aq) 1.00 x 10-² 8.00 x 10-³ -1.00 x 10-² -8.00 x 10-³ NEXT H₂NNH3 + (aq) 2.00 x 10-³ RESET -2.00 × 10-³ +

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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 107AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...
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A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. NEXT > 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 100 mL of 0.100 M HNO3 (a strong acid). Fill in the BCA 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.. Before (mol) Change (mol) After (mol) 6.00 × 10-³ 0 -6.00 × 10-³ 1 H₂NNH₂(aq) 0.100 7.00 × 10-3 0.200 -7.00 × 10-³ + H+ (aq) 1.00 x 10-² 2 8.00 × 10-³ -1.00 x 10-² -8.00 × 10-³ H₂NNH3 + (aq) 2.00 × 10-³ RESET -2.00 × 10-³ +
Transcribed Image Text:A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. NEXT > 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 100 mL of 0.100 M HNO3 (a strong acid). Fill in the BCA 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.. Before (mol) Change (mol) After (mol) 6.00 × 10-³ 0 -6.00 × 10-³ 1 H₂NNH₂(aq) 0.100 7.00 × 10-3 0.200 -7.00 × 10-³ + H+ (aq) 1.00 x 10-² 2 8.00 × 10-³ -1.00 x 10-² -8.00 × 10-³ H₂NNH3 + (aq) 2.00 × 10-³ RESET -2.00 × 10-³ +
< PREV The value of Kb for H₂NNH₂ is 3.0 x 10-6. Based on the result of the acid-base reaction, determine the pH of this final solution. 0 A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. 10.1 6.21 12.3 1 7.79 3.70 pH = 11.3 17.7 2.70 2 1.85 1.70 RESET 3.91
Transcribed Image Text:< PREV The value of Kb for H₂NNH₂ is 3.0 x 10-6. Based on the result of the acid-base reaction, determine the pH of this final solution. 0 A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. 10.1 6.21 12.3 1 7.79 3.70 pH = 11.3 17.7 2.70 2 1.85 1.70 RESET 3.91
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