Determine the pH at the point in the titration of 40.0 mL of 0.200 MH2NNH2 with 0.100 M HNO: after 80.0 mL of the strong acid has beenadded. The value of Kb for H2NNH2 is 3.0 x 106.3.4NEXT >Use the table below to determine the moles of reactant and product after the reaction ofthe acid and base.H2NNH:(aq)H(aq)H2NNH3*(aq)->Before (mol)Change (mol)After (mol)↑ Determine the pH at the point in the titration of 40.0 mL of 0.200 MH2NNH2 with 0.100 M HNO: after 80.0 mL of the strong acid has beenadded. The value of Kb for H2NNH2 is 3.0 x 10 6,NEXT >K PREV1Based on the result of the acid-base reaction, set up the ICE table in order to determinethe unknown.H2O(I)1LH:O*(aq)+ H¿NNH2(aq)H2NNH3*(aq) +Initial (M)Change (M)Equilibrium(M)RESET3.

Given: volume of NH2NH2 = 40.0 mL Molarity of NH2NH2 = 0.200 M volume of HNO3 = 80.0 mL Molarity of…

Answered: Determine the pH at the point in the…

Determine the pH at the point in the titration of 40.0 mL of 0.200M H2NNH2 with 0.100 M HNO: after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10 6.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Determine the pH at the point in the titration of 40.0 mL of 0.200 M
H2NNH2 with 0.100 M HNO: after 80.0 mL of the strong acid has been
added. The value of Kb for H2NNH2 is 3.0 x 106.
3.
4
NEXT >
Use the table below to determine the moles of reactant and product after the reaction of
the acid and base.
H2NNH:(aq)
H(aq)
H2NNH3*(aq)
->
Before (mol)
Change (mol)
After (mol)
↑

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