2. For each titration, predict whether the equivalence point is less than, equal to, or greater thanpH = 7. (Circle)a) Pyridine (CSH5N) titrated with nitric acidb) Acetic acid titrated with calcium hydroxide< pH 7< pH 7< pH 7> pH 7> pH 7> pH 7= pH 7= pH 7c) Hydrobromic acid titrated with strontium hydroxide= pH 73. Calculate the pH at 25°C of a solution that results from mixing equal volumes of a 0.050 M solution ofammonia and a 0.025 M solution of hydrochloric acid? pKa(NH4*) is 9.25.

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For each titration, predict whether the equivalence point is less than, equal to, or greater than pH = 7. (Circle)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.29QAP

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Ionic Equilibrium

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.

Question

2. For each titration, predict whether the equivalence point is less than, equal to, or greater than
pH = 7. (Circle)
a) Pyridine (CSH5N) titrated with nitric acid
b) Acetic acid titrated with calcium hydroxide
< pH 7
< pH 7
< pH 7
> pH 7
> pH 7
> pH 7
= pH 7
= pH 7
c) Hydrobromic acid titrated with strontium hydroxide
= pH 7
3. Calculate the pH at 25°C of a solution that results from mixing equal volumes of a 0.050 M solution of
ammonia and a 0.025 M solution of hydrochloric acid? pKa(NH4*) is 9.25.

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