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 thisinformation 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 ICEtable with the appropriate value for each involved species to determine the moles of reactant and productafter 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 10Initial (M)Change (M)Equilibrium (M)-X0.140-x0-6.00 x 10³0110.200 + xH₂NNH₂(aq)0.2000.175 + x7.00 x 10³H₂NNH₂(aq) +20.2000.200 - x0.175-x0.1002-7.00 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 thisinformation to determine the pH. Complete Parts 1-4 before submitting your answer.< PREV3Upon completion of the acid-base reaction, the H₂NNH3* ion is in equilibrium with water. Set up the ICEtable in order to determine the unknown concentrations of reactants and products..+0.0200H₂O(l)0.0200 + x31.00 x 10"8.00 × 10³0.100H*(aq)0.0200 - x-1.00 x 10"-8.00 × 10³4OH(aq)0.1402.00 x 100.100 + x4H₂NNH3 + (aq)0.175RESET-2.00 x 10"0.100 - x+ H₂NNH3*(aq)NEXTRESET+x0.140 + 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 thisinformation to determine the pH. Complete Parts 1-4 before submitting your answer.< PREV123NEXT >The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set upthe expression for Kb in order to determine the unknown concentrations. Each reaction participant must berepresented 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 =14.77 x 10-1⁰12.3[0.0200][0.0200 + x] [0.0200 -x][0.100]10.82[0.140][0.100 + x]2.10 x 10-5A 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 thisinformation to determine the pH. Complete Parts 1-4 before submitting your answer.= 3.0 x 10-6< PREVsed 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]49.32[x][0.140 + x]4RESET[2x]3.22[0.140 -x]RESET0.140

Answered: Image /qna-images/answer/a0539434-b4f6-4fc3-91e8-74bff9f5efe2.jpg

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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 111QRT: Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong...

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