[H+] in concentrated buffer Put your answer here with units! Use Equation editor here to show all your work! You can copy and paste these when you need more lines [H+] in diluted buffer Put your answer here with units! Use Equation editor here to show all your work! You can copy and paste these when you need more lines Average [H+] in buffer, which is equal to the average Ka for ammonium
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.
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![Table 1 - Indicator Colors when Measuring 0.1 M Acetic Acid (CH3CO2H)
Part A - indicators
Indicator
methyl violet
thymol blue
brilliant red
methyl orange
bromaccesal green
bromothymol blue
Solution sample
sodium carbonate
sodium hydrogen sulfate
Table 2 - pH Meter Measurement of Various 0.1 M Solutions
Part B - pH meters
acetic acid
sodium acetate
zinc sulfate
pH of concentrated buffer
pH of diluted buffer
pH of buffer + HCL
pH of buffer + NaOH
Color
Royal dark purple
Sunshine orange
Super dark purple
Cotton candy pink
pH of pure water
Lemon yellow
Amber yellow
pH of water + HCI
pH of water + NaOH
pH
11.95
1.00
Table 3 - pH Meter Measurement Values of Ammonia/Ammonium Buffer
Part C - Buffers
2.65
7.10
5.11
9.60
9.36
Table 4 - pH Meter Measurement Value of Non-Buffered Solutions
Part D - Comparison to water
9.32
9.45
10.02
5.42
6.29
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![4) Calculate the [H+] from both the concentrated buffer and diluted buffer in Part
C. In this case, these concentrations are the Ka of the ammonium. Report the
average Ka for ammonium. For these calculations, you will be required to
show detailed work steps using Equation Editor or similar.
Use Equation editor here to show all your work! You can copy and paste these when you need more lines
[H+] in concentrated buffer
Put your answer here with units!
Use Equation editor here to show all your work! You can copy and paste these when you need more lines
[H+] in diluted buffer
Put your answer here with units!
Use Equation editor here to show all your work! You can copy and paste these when you need more lines
Average [H+] in buffer, which is equal to the average Ka for ammonium
Put your answer here!
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