Friday, October 4, 2013
WRITING TASKS:
1. Identify what subject you are exploring (including your focal play). Why is this subject interesting? What do you hope to discover?
2. Neatly summarize the plots, characters and themes of one play (not one which you describe in a Short Play Report).
3. Pick 3 different articles to summarize and evaluate:
1. You need a researchable topic or question, and 3 likely and substantial articles related to it. (Vary search terms & engines as needed. Appropriate websites or webpages: essays, reviews, history, definitions, etc. Not cinematographic background ‘news’ or mere reports of new movies.)
2. Give a full citation (MLA format) for each article. Cite EACH of your THREE sources fully: Web addresses are to be included–but they are NOT enough.
3. Summarize what each article says: what was its thesis statement or question, in what parts or steps did the author develop his thesis, and what kind of supporting evidence did he bring to bear? Summarize what is important about each webpage (–and its host website), including specifics on the topic and how it is developed, explanation of point of view and/or purpose, the format of the webpage, the quantity and quality of background links, and at least one distinctive example.
4. Then critique each article separately: what was interesting or well done in each essay, and what fell short of satisfying us? Critique the A) writing, B) usefulness, and C) informativeness of each article.
5. Post your reviews in 3 entries, with two bullets or numbered paragraphs in each entry.
6. Identify also, finally, which article is the best (and which the worst), and explain why.
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Half Titration
Determining Ka by the
Half-Titration of a Weak Acid
A common analysis of a weak acid or a weak base is to conduct a titration with a base or acid of known molar concentration to help determine the equilibrium constant, Ka, for the weak acid or weak base. If this titration is conducted very carefully and very precisely, the results can lead to a valid approximation of an equilibrium constant. In this experiment, however, you will use a different technique to determine the Ka for a weak acid, acetic acid.
Your primary goal in this experiment is to calculate the Ka of acetic acid. The data that you will use to complete your calculations will come from the reaction of acetic acid with a solution of NaOH. Recall from your work with weak acid-strong base titrations that the point at which a reaction is half-titrated can be used to determine the pKa of the weak acid. In this experiment, the half-titration point will exist when you have added half as many moles of HC2H3O2 as moles of NaOH . Thus, OH– will have reacted with half of the HC2H3O2, leaving the solution with equal moles of HC2H3O2 and C2H3O2 –. At this point, according to the Henderson-Hasselbalch equation,
Half-Titration of a Weak Acid
A common analysis of a weak acid or a weak base is to conduct a titration with a base or acid of known molar concentration to help determine the equilibrium constant, Ka, for the weak acid or weak base. If this titration is conducted very carefully and very precisely, the results can lead to a valid approximation of an equilibrium constant. In this experiment, however, you will use a different technique to determine the Ka for a weak acid, acetic acid.
Your primary goal in this experiment is to calculate the Ka of acetic acid. The data that you will use to complete your calculations will come from the reaction of acetic acid with a solution of NaOH. Recall from your work with weak acid-strong base titrations that the point at which a reaction is half-titrated can be used to determine the pKa of the weak acid. In this experiment, the half-titration point will exist when you have added half as many moles of HC2H3O2 as moles of NaOH . Thus, OH– will have reacted with half of the HC2H3O2, leaving the solution with equal moles of HC2H3O2 and C2H3O2 –. At this point, according to the Henderson-Hasselbalch equation,
if there are equal moles of HC2H3O2 and C2H3O2 – at the half-titration point, then pKa is equal to the pH value of the solution.
In this experiment, you may find it surprising that you do not need to keep close track of the volume of NaOH titrant added, as you would in most titrations. It is also unusual to conduct a titration without plotting or analyzing a conventional titration curve. This is the nature of a half-titration; it is only important to know when equal amounts of OH– and HC2H3O2 have been added.CLICK HERE TO GET MORE ON THIS PAPER.....
In this experiment, you may find it surprising that you do not need to keep close track of the volume of NaOH titrant added, as you would in most titrations. It is also unusual to conduct a titration without plotting or analyzing a conventional titration curve. This is the nature of a half-titration; it is only important to know when equal amounts of OH– and HC2H3O2 have been added.CLICK HERE TO GET MORE ON THIS PAPER.....
OBJECTIVES
In this experiment, you will
• Conduct a reaction between solutions of a weak acid and sodium hydroxide.
• Determine the half-titration point of an acid-base reaction.
• Calculate the Ka and pKa for the weak acid.
Figure 1
MATERIALS
LabQuest 1.00 M sodium hydroxide, NaOH, solution
LabQuest App 1.00 M acetic acid, HC2H3O2, solution
Vernier pH Sensor phenolphthalein indicator solution
50 mL buret distilled water
buret clamp magnetic stirrer and stirring bar
250 mL beaker plastic Beral pipets
two ring stands utility clamp
PROCEDURE
1. Obtain and wear goggles.
2. Use a buret clamp to connect a 50 mL buret to a ring stand. Rinse and fill the buret with
1.00 M acetic acid solution. Handle the acetic acid with care. It can cause painful burns if it comes into contact with the skin.
3. Transfer precisely 25.0 mL of the acetic acid solution to a 250 mL beaker.
4. Use a plastic Beral pipet to remove a small volume of the acetic acid from the 250 mL beaker. Draw enough acetic acid into the pipet so that the bulb is about 1/4 full. Carefully set aside the pipet of acid, to be used later.
5. Add 1–2 drops of phenolphthalein indicator solution to the beaker of acetic acid.
6. Connect the pH Sensor to LabQuest and choose New from the File menu. If you have an older sensor that does not auto-ID, manually set up the sensor.
7. Obtain about 50 mL of 1.00 M NaOH solution. CAUTION: Sodium hydroxide solution is caustic. Avoid spilling it on your skin or clothing.
8. Begin the half-titration.
a. Place the beaker of acetic acid on a magnetic stirrer and add a stirring bar.
b. Set up a ring stand and clamp to hold the pH Sensor in place (see Figure 1). Position the pH Sensor in the beaker so that the tip of the probe is completely immersed.
c. Gently stir the acetic acid solution.
d. Do not start data collection. Monitor the pH of the reaction mixture on LabQuest.
e. Use a new plastic Beral pipet to slowly add the 1.00 M NaOH solution, in ~1 mL increments, to the beaker of acetic acid solution (see Figure 1).
In this experiment, you will
• Conduct a reaction between solutions of a weak acid and sodium hydroxide.
• Determine the half-titration point of an acid-base reaction.
• Calculate the Ka and pKa for the weak acid.
Figure 1
MATERIALS
LabQuest 1.00 M sodium hydroxide, NaOH, solution
LabQuest App 1.00 M acetic acid, HC2H3O2, solution
Vernier pH Sensor phenolphthalein indicator solution
50 mL buret distilled water
buret clamp magnetic stirrer and stirring bar
250 mL beaker plastic Beral pipets
two ring stands utility clamp
PROCEDURE
1. Obtain and wear goggles.
2. Use a buret clamp to connect a 50 mL buret to a ring stand. Rinse and fill the buret with
1.00 M acetic acid solution. Handle the acetic acid with care. It can cause painful burns if it comes into contact with the skin.
3. Transfer precisely 25.0 mL of the acetic acid solution to a 250 mL beaker.
4. Use a plastic Beral pipet to remove a small volume of the acetic acid from the 250 mL beaker. Draw enough acetic acid into the pipet so that the bulb is about 1/4 full. Carefully set aside the pipet of acid, to be used later.
5. Add 1–2 drops of phenolphthalein indicator solution to the beaker of acetic acid.
6. Connect the pH Sensor to LabQuest and choose New from the File menu. If you have an older sensor that does not auto-ID, manually set up the sensor.
7. Obtain about 50 mL of 1.00 M NaOH solution. CAUTION: Sodium hydroxide solution is caustic. Avoid spilling it on your skin or clothing.
8. Begin the half-titration.
a. Place the beaker of acetic acid on a magnetic stirrer and add a stirring bar.
b. Set up a ring stand and clamp to hold the pH Sensor in place (see Figure 1). Position the pH Sensor in the beaker so that the tip of the probe is completely immersed.
c. Gently stir the acetic acid solution.
d. Do not start data collection. Monitor the pH of the reaction mixture on LabQuest.
e. Use a new plastic Beral pipet to slowly add the 1.00 M NaOH solution, in ~1 mL increments, to the beaker of acetic acid solution (see Figure 1).
9. Conduct the titration carefully. As the reaction approaches the equivalence point, at about pH 6, add the NaOH solution drop by drop. When you reach the equivalence point, the pH will increase rapidly and the indicator will change color. If necessary, add another drop of NaOH, so that the reaction is slightly past the equivalence point. Remember that the pH will not increase rapidly beyond the equivalence point (pH ~10).
10. Add all of the acetic acid from the Beral pipet, which you removed in Step 4, to the beaker of reaction mixture. Check the pH readings and observe the indicator color. The mixture should be slightly acidic once again.
11. Carefully add NaOH, drop by drop, to the beaker of reaction mixture, until you reach the equivalence point as precisely as possible. A very slight pink color of the phenolphthalein indicator is visible. This is your half-titrated solution, because you have neutralized precisely 25.0 mL of the original 50.0 mL of acetic acid that you measured out into the buret.
12. Transfer the remaining 25.0 mL of acetic acid from the buret to the 250 mL beaker of reaction mixture. Stir the solution in the beaker thoroughly. Read and record the pH of the solution in the beaker.
13. When you have finished the testing, dispose of the reaction mixture as directed. Rinse the pH Sensor with distilled water in preparation for a second trial. Repeat the necessary steps to test a new sample of the acetic acid solution.
10. Add all of the acetic acid from the Beral pipet, which you removed in Step 4, to the beaker of reaction mixture. Check the pH readings and observe the indicator color. The mixture should be slightly acidic once again.
11. Carefully add NaOH, drop by drop, to the beaker of reaction mixture, until you reach the equivalence point as precisely as possible. A very slight pink color of the phenolphthalein indicator is visible. This is your half-titrated solution, because you have neutralized precisely 25.0 mL of the original 50.0 mL of acetic acid that you measured out into the buret.
12. Transfer the remaining 25.0 mL of acetic acid from the buret to the 250 mL beaker of reaction mixture. Stir the solution in the beaker thoroughly. Read and record the pH of the solution in the beaker.
13. When you have finished the testing, dispose of the reaction mixture as directed. Rinse the pH Sensor with distilled water in preparation for a second trial. Repeat the necessary steps to test a new sample of the acetic acid solution.
DATA TABLE
Titration Results Trial 1 Trial 2
Equivalence point pH 8.68 8.25
pH of half-titrated solution 4.84 4.77
DATA ANALYSIS
1. Calculate the pKa and Ka using the results of your testing.
2. Find the accepted values for the pKa and Ka of acetic acid. How well do the accepted values compare with your calculated values? Explain.
3. Explain why the pH at the half-titration point is equal to the pKa in your experiment.
4. Explain how this test could be done using only an indicator solution and no electronic means of measuring pH.
Titration Results Trial 1 Trial 2
Equivalence point pH 8.68 8.25
pH of half-titrated solution 4.84 4.77
DATA ANALYSIS
1. Calculate the pKa and Ka using the results of your testing.
2. Find the accepted values for the pKa and Ka of acetic acid. How well do the accepted values compare with your calculated values? Explain.
3. Explain why the pH at the half-titration point is equal to the pKa in your experiment.
4. Explain how this test could be done using only an indicator solution and no electronic means of measuring pH.
Academic and Professional Development (Summary and Critically Analyse)
What is a summary?
It is an overview of the research method.. was it a qualitative or a quantitative research? Pulling out the important points.. It’s like an abstract!
Please Summarise the first document which is under the name of (UNDERSTANDING STUDENT PLAGIARISM) in 250 words ONLY! (Only summarise the key findings and the methodology).
Then Analyse the work in 750 words ONLY! And do NOT summarise the journal again! However, compare and contrast the (Understanding student plagiarism) journal article with the other journal articles that I have attached on the topic .. please use them all and mention the authors names within the body paragraphs! and reference them well.
1. Summarise the paper IN YOUR OWN WORDS. Do not just repeat the abstract (250 words).
2. Critically analyse the paper’s purpose. You should aim to cover the following: What is being reported and why? What are its strengths? Are there any weaknesses? Was the methodology appropriate? What questions does it raise? How does it fit with current (after 2011) thinking on the subject of plagiarism?
Your critique must be underpinned with scholarly work and academic thinking. Do not base it on your own opinion or unverified internet sources. You must use appropriate citations in your text and list the references used, alphabetically, at the end of your critique, using MMUBS Harvard referencing (750 words). You must use formal academic English that is without abbreviations, colloquialisms or vernacular.
Please note this critique is not about the author’s ability to write an academic paper or how it is structured it is about the contents, the purpose and the strength of the research being reported.
Total word count – 1,000 words
Please note this critique is not about the author’s ability to write an academic paper or how it is structured it is about the contents, the purpose and the strength of the research being reported.
Total word count – 1,000 words
Respondeat Superior
Discuss Respondeat Superior including the following components:
• Introduction that includes the thesis statement (Content criteria #1)
• Describe the meaning of the legal doctrine, Respondeat Superior. (Content criteria #2)
• Provide at least two examples of cases where the doctrine was applied and analyze whether or not the doctrine was applied fairly to each of the examples. (content criteria #3)
• Conclusion (included in #1)
• Describe the meaning of the legal doctrine, Respondeat Superior. (Content criteria #2)
• Provide at least two examples of cases where the doctrine was applied and analyze whether or not the doctrine was applied fairly to each of the examples. (content criteria #3)
• Conclusion (included in #1)
Molar Solutions used in Nursing Profession
In your text in chapter 2 (Text Book ISBN#10:0-321-80928-9, 13:978-0-321-80928-5) it desribes how to make a molar solution and a solution that is a percentage mass by mass or a percentage volume by volume. Find a solution you will use in your occupation "Nursing Profession." Write the procedures for how you would make the solution and how you determined the numbers for the volumes or masses needed to make the solution. Describe if the solution’s concentration has units of M, %m/m, or %v/v. What is the solvent and what is the solute? Is the solvent polar, nonpolar, or ionic? Is the solute polar, nonpolar, or ionic? Is the solution an electrolyte, weak electrolyte, or nonelectrolyte?
Based on the description of your solution above how does the solution work in the system in which you will place it? What reactions, solubilities, or electrolytic properties become important in the system? How does limiting reactant, theoretical yield, actual yield, and percentage yield work in the system you are creating?
dramatic’ human condition
1. Analyze Nora’s problem, and Nora’s role in that problem. Use support from the play.
2. Analyze Ms. Warren’s problem, and determine its causes. Use support from the play.
3. What is the trick of ‘six characters who need (?) to search for an author’ — and why does Pirandello dramatize this ‘dramatic’ human condition?
4. What is the meaning of Wilson’s fences? Illustrate.
5. Which part of the reading or lecture is foggiest?
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