This document provides an overview of applying equilibrium concepts to acid-base chemistry. It discusses the common ion effect, buffered solutions, calculating pH of buffers using the Henderson-Hasselbach equation, effects of adding strong acids/bases to solutions, buffer capacity, and titration curves. Key points include:
- The common ion effect lowers the dissociation of a weak acid/base when a salt containing its ion is added
- Buffered solutions resist pH changes due to a mixture of weak acid/base and its salt
- The H-H equation can be used to calculate pH of buffer solutions
- Adding a strong base/acid may react with and reduce the concentration of the conjugate acid/base of a buffer
Application of Statistical and mathematical equations in Chemistry Part 5Awad Albalwi
Application of Statistical and mathematical equations in Chemistry
Part 5
Strong Acids and Bases
Ph theory
Weak Acids and Weak Bases
Salts of Weak Acids and Bases theory
A buffer solution theory
POLYPROTIC ACID IONIZATION
Application of Statistical and mathematical equations in Chemistry Part 5Awad Albalwi
Application of Statistical and mathematical equations in Chemistry
Part 5
Strong Acids and Bases
Ph theory
Weak Acids and Weak Bases
Salts of Weak Acids and Bases theory
A buffer solution theory
POLYPROTIC ACID IONIZATION
Module
Analytical Measurement
Tutor
Code
ICA
Excel simulation of a titration involving strong acid and a weak base (or v.v.)
2nd Marker
Weight
50%
Type
Online submission
Produce an Excel spreadsheet based on simulation to illustrate the variation of the pH of the solution that occurs when strong acid is added to a weak base (or strong alkali and weak acid). The spreadsheet should demonstrate the change in the pH of the mixture as the titrant is added for a range of concentration of both components. Particular attention should be paid to the behaviour close to the end point (or equivalence point). Graphs should be generated on a range of scales showing in detail the likely behaviour around the end point.
The exact calculations for all situations can be quite involved so it may be useful to divide the titration into various segments in which various equations and approximations are valid and then stitch these together.
Write a report explaining the design of your spreadsheet and describe the graphs, which you should import.
Write a short description of the theory of buffer solutions and give examples of their applications.
The report should be a word document and an Excel spreadsheet. Describe the background theory and the methodology behind the construction of the simulation, and include the realisation of the system equations in Excel formulae. Graphs of pH against added solution over various ranges and around particular key points – such as the equivalence point or “end point”.
[60 marks]
The report should also include a discussion of the concept of buffer solutions and give examples of their use either in industrial processes or naturally occurring phenomena. Any sources should be appropriately referenced (Harvard).
[40 marks]
assignhints(1).pptx
Hints for the Assignment Weak Monoprotic AcidsNameFormulaValue of KaMonochloracetic acid
Hydrofluoric acid
Nitrous acid
Formic acid
Lactic acid
Benzoic acid
Acetic acid
Hydrated aluminum(III) ion
Propanoic acid
Hypochlorous acid
Hypobromous acid
Hvdrocyanic aid
Boric acid
Ammonium ion
Phenol HC2H3ClO2
HF
HNO2
HCO2H
HC3H5O3
HC7H502
HC2H3O2
[Al (H20)6]3+
HC3H5O2
HOCl
HOBr
HCN
H3BO3
NH4+
HOC6H5
HOI 1.35 x 10 -3
7.2 x 10-4
4.0 x 10-4
1.8 x 10-4
1.38 x 10-4
6.4 x 10-5
1.8 x 10-5
1.4 x 10-5
1.3 x 10-5
3.5 x 10-8
2 x 10-9
6.2 x 10-10
5.8 x 10-10
5.6 x 10-10
1.6 x 10-10
2 x 10-11
Weak Alkalis or BasesFormulaNameKbNH3ammonia
1.8 x 10 -5CH3NH2methylamine
4.4 x 10 -4C5H5Npyridine
1.5 x 10 -9C6H5NH2aniline4.3 x 10 -10
It is possible to set up a simulated titration between a weak acid and a strong base.
It is easier to work backwards from pH to the added volume of titrant using the equations below as [H+] = 10(-pH)
It is possible to generate the curve with just one formula going backwards.
However we know by working forwards from added volume to pH that there are certain key points of interest, namely where φ = 0, 0.5, 1 and >1.
...
Module
Analytical Measurement
Tutor
Code
ICA
Excel simulation of a titration involving strong acid and a weak base (or v.v.)
2nd Marker
Weight
50%
Type
Online submission
Produce an Excel spreadsheet based on simulation to illustrate the variation of the pH of the solution that occurs when strong acid is added to a weak base (or strong alkali and weak acid). The spreadsheet should demonstrate the change in the pH of the mixture as the titrant is added for a range of concentration of both components. Particular attention should be paid to the behaviour close to the end point (or equivalence point). Graphs should be generated on a range of scales showing in detail the likely behaviour around the end point.
The exact calculations for all situations can be quite involved so it may be useful to divide the titration into various segments in which various equations and approximations are valid and then stitch these together.
Write a report explaining the design of your spreadsheet and describe the graphs, which you should import.
Write a short description of the theory of buffer solutions and give examples of their applications.
The report should be a word document and an Excel spreadsheet. Describe the background theory and the methodology behind the construction of the simulation, and include the realisation of the system equations in Excel formulae. Graphs of pH against added solution over various ranges and around particular key points – such as the equivalence point or “end point”.
[60 marks]
The report should also include a discussion of the concept of buffer solutions and give examples of their use either in industrial processes or naturally occurring phenomena. Any sources should be appropriately referenced (Harvard).
[40 marks]
assignhints(1).pptx
Hints for the Assignment Weak Monoprotic AcidsNameFormulaValue of KaMonochloracetic acid
Hydrofluoric acid
Nitrous acid
Formic acid
Lactic acid
Benzoic acid
Acetic acid
Hydrated aluminum(III) ion
Propanoic acid
Hypochlorous acid
Hypobromous acid
Hvdrocyanic aid
Boric acid
Ammonium ion
Phenol HC2H3ClO2
HF
HNO2
HCO2H
HC3H5O3
HC7H502
HC2H3O2
[Al (H20)6]3+
HC3H5O2
HOCl
HOBr
HCN
H3BO3
NH4+
HOC6H5
HOI 1.35 x 10 -3
7.2 x 10-4
4.0 x 10-4
1.8 x 10-4
1.38 x 10-4
6.4 x 10-5
1.8 x 10-5
1.4 x 10-5
1.3 x 10-5
3.5 x 10-8
2 x 10-9
6.2 x 10-10
5.8 x 10-10
5.6 x 10-10
1.6 x 10-10
2 x 10-11
Weak Alkalis or BasesFormulaNameKbNH3ammonia
1.8 x 10 -5CH3NH2methylamine
4.4 x 10 -4C5H5Npyridine
1.5 x 10 -9C6H5NH2aniline4.3 x 10 -10
It is possible to set up a simulated titration between a weak acid and a strong base.
It is easier to work backwards from pH to the added volume of titrant using the equations below as [H+] = 10(-pH)
It is possible to generate the curve with just one formula going backwards.
However we know by working forwards from added volume to pH that there are certain key points of interest, namely where φ = 0, 0.5, 1 and >1.
...
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http://sandymillin.wordpress.com/iateflwebinar2024
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The Art Pastor's Guide to Sabbath | Steve ThomasonSteve Thomason
What is the purpose of the Sabbath Law in the Torah. It is interesting to compare how the context of the law shifts from Exodus to Deuteronomy. Who gets to rest, and why?
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52. Titration Curve for Weak Acid & Strong Base Over what pH range does the titrated solution suddenly change from high [H 3 O 1+ ] to high [OH 1- ]? About 6.5 to 11 What’s pH when 0.067 mol NaOH added? pH = 5 What’s [H 3 O 1+ ]? [H 3 O 1+ ] = 1 x 10 -5 M Best Indicator (p. 756 & next slide)? o -Cresolphthalein or Phenolphthalein.
60. Figure 15.8 p. 756: The Useful pH Ranges for Several Common Indicators
61. Color Ranges of Various Indicators Used in Titrations Why are different indicators used for SA-SB, SA-WB, or WA-SB titrations? Each type of titration has a different end point. Is it better to use an indicator with a color change over a wide or narrow pH range. Why? Narrow pH range since gives better approximation of the end point.
62. pH Scale Relationships If [H 3 O 1+ ] of “x” is 10 x greater than another with pH 3, what is pH of “x”? pH = 2 If [OH 1- ] of “y” is 1000 x greater than pure water’s, what is pH of “y”? pH = 10 Is hand soap more or less basic than baking soda? More basic.
63. Figure 15.9 p. 757 The pH Curve for the Titration of 100.0 mL of 0.10 M HCI with 0.10 M NaOH Which is the better indicator? Neither, since their ranges are not close to the equivalence (end) point.
64. Figure 15.10 p. 757 The pH Curve for the Titration of 50 mL of 0.1 M HC 2 H 3 O 2 with 0.1 M NaOH Choose the best indicator between the two . . . Phenolphthalein
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