The following graph was produced using the data collected in the second part of the lab. Answer the questions below based on the videos and graph provided. Strong Bases/Acids vs. Weak Bases/Acids The 4 Titration Curves · Combinations NaOH + HCI Strong Base Strong Acid NaOH + CH,COOH Strong Base Weak Acid NH,OH + HCI Weak Base Strong Acid NH.OH + CH;COOH Weak Base Weak Acid Explain why two titrations started at a higher pH value and two titrations started at a lower pH value, yet each titration started with the same concentration for the acid. What was the purpose of adding the indicator to each titration? Two titrations ended with the pH well above 10 the other two titrations ended with the pH below 10. Explain why this occurred. A common mistake made by chemistry students is assuming that all acid base neutralization reactions will have an equivalence point at a pH of 7.0. Using the results from the lab, explain why this is not true. Your answer needs to include all four titrations' results. F.
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.
Please give answer of the question-F accurate and exact with detailed and complete reasons it must be detailed solution please. I'll rate. Thanks
(Only last part-F) detailed solution please
![The following graph was produced using the data collected in the second part of the lab. Answer the
questions below based on the videos and graph provided.
Strong Bases/Acids vs. Weak Bases/Acids
The 4 Titration Curves Combinations
N2OH + HCI
Strong Base + Strong Acid
NaOH + CH,COOH
Strong Base + Weak Acid
NH,OH + HCI
Weak Base + Strong Acid
NH.OH + CH;COOH
Weak Base Weak Acid
200
1427, 102)
Explain why two titrations started at a higher pH value and two titrations started at a lower pH
value, yet each titration started with the same concentration for the acid.
What was the purpose of adding the indicator to each titration?
Two titrations ended with the pH well above 10 the other two titrations ended with the pH
below 10. Explain why this occurred.
A common mistake made by chemistry students is assuming that all acid base neutralization
F.
reactions will have an equivalence point at a pH of 7.0. Using the results from the lab, explain
why this is not true. Your answer needs to include all four titrations' results.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2e070b2-938d-48db-a325-7001f88c0299%2Fd186bf7d-c32a-48a1-b70f-2892da6b753f%2Fjuuhpif_processed.jpeg&w=3840&q=75)
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