1011121314An analytical chemist is titrating 234.9 mL of a 0.2700M solution of ethylamine (C,H,NH,) with a 0.1500M solution of HNO2. The p K, of ethylamine is 3.19.Calculate the pH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it.Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.Round your answer to 2 decimal places.pH =|Submit AssignmentContinue

Given, Molarity of base =0.270 M Volume of Base = 234.9 mL Mmol of Base = M × V = 234.9 × 0.27 =…

DH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it. db nced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. answer to 2 decimal places. Submit Assignment

DH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it. db nced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. answer to 2 decimal places. Submit Assignment

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 55P

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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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An analytical chemist is titrating 234.9 mL of a 0.2700M solution of ethylamine (C,H,NH,) with a 0.1500M solution of HNO2. The p K, of ethylamine is 3.19.
Calculate the pH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.
Round your answer to 2 decimal places.
pH =|
Submit Assignment
Continue

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