Calculate the starting concentration of your unknown acid solution.CExplain why the pH at the equivalence point is not 7, the pH of neutral water. From your graph, determine the pH and volume of base added at the equivalence point. Determine the point which should correspond to the pKa of your acid and determine what your Ka should be. What ions and molecules are present in the solution at the point when half of the volume of base at the equivalence point has been added? How does this compare to a point with double the volume of base compared to the equivalence point? Identify which acid you believe you have and provide your reasoning. For your identified acid, write the balanced chemical equation for the neutralization reaction you performed. Write the Ka expression for your acid. Calculate the [H3O+] concentration of your acid before any base is added assuming a starting concentration of 0.685 M using an ICE table. Determine the % ionization of your acid before any base is added. Determine the mass of acid you would have needed to add to the 25.00 mL of water in order to create the solution in #9 Assuming you want to turn the solution from #9 into an ideal buffer solution, approximately what mass of the 2nd buffer

Calculate the starting concentration of your unknown acid solution.CExplain why the pH at the equivalence point is not 7, the pH of neutral water. From your graph, determine the pH and volume of base added at the equivalence point. Determine the point which should correspond to the pKa of your acid and determine what your Ka should be. What ions and molecules are present in the solution at the point when half of the volume of base at the equivalence point has been added? How does this compare to a point with double the volume of base compared to the equivalence point? Identify which acid you believe you have and provide your reasoning. For your identified acid, write the balanced chemical equation for the neutralization reaction you performed. Write the Ka expression for your acid. Calculate the [H3O+] concentration of your acid before any base is added assuming a starting concentration of 0.685 M using an ICE table. Determine the % ionization of your acid before any base is added. Determine the mass of acid you would have needed to add to the 25.00 mL of water in order to create the solution in #9 Assuming you want to turn the solution from #9 into an ideal buffer solution, approximately what mass of the 2nd buffer

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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

I
Calculate the starting concentration of your unknown acid solution.CExplain why the pH at the equivalence
point is not 7, the pH of neutral water. From your graph, determine the pH and volume of base added at
the equivalence point. Determine the point which should correspond to the pka of your acid and
determine what your Ka should be. What ions and molecules are present in the solution at the point when
half of the volume of base at the equivalence point has been added? How does this compare to a point
with double the volume of base compared to the equivalence point? Identify which acid you believe you
have and provide your reasoning. For your identified acid, write the balanced chemical equation for the
neutralization reaction you performed. Write the Ka expression for your acid. Calculate the [H3O+]
concentration of your acid before any base is added assuming a starting concentration of 0.685 M using an
ICE table. Determine the % ionization of your acid before any base is added. Determine the mass of acid
you would have needed to add to the 25.00 mL of water in order to create the solution in #9 Assuming you
want to turn the solution from #9 into an ideal buffer solution, approximately what mass of the 2nd buffer
component would you need to add (assume the potassium salt)?
Weak Acid-Strong Base Titration Graph
Hd
15
10
5
0
3
10
NaOH (mL)
20
30

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