Literary Analysis of Shakespeares Twelfth Night Essay

Shakespeare’s Twelfth Night is a play with themes that parallel the folly of the festival it is named after. The main storyline of the plot plays on this a lot by mixing up the stereotypes around gender that were very present at the time. However, a sub-plot involving secondary characters defines this theme even more. It takes the idea even further by relating servants’ attempts to blur the lines between social classes. Twelfth Night’s Maria and Malvolio both have great aspirations to rise above their social class. However, Maria succeeds where Malvolio fails because of her capability to make use of the satiric ambiance of her mistress’s household to achieve her goals. To begin this essay, I will provide a brief analysis of the†¦show more content†¦In Shakespeare’s play, Malvolio and Maria both wish to do this; one by courting Olivia, and the other by trying to get closer to Sir Toby. The main difference between the two characters is Malvolio’s self-adulation and lust for power in comparison of Maria’s cleverness and her willingness to put her immediate wants aside to ultimately satisfy her craving for a better social standing at a later time. Malvolio’s immediate addiction to power and wish to get revenge on others overcomes any will he could have to play a part to access a higher social status. While some may think that Malvolio is essentially a moral and just person, this can be disproved by shedding more light on his less-honourable practices, like his abuse of power. Essentially, like it is pointed out even by her mistress (INSERT QUOTE), Malvolio is just an extensively pompous person. Personality-wise, his narcistic and patronizing ways are made to recall those of a nobleman. These traits fit in easily with his character, as he obviously aspires to be part Illyria’s nobility one day (INSERT QUOTE). The essence of Malvolio’s personality is ascertained by Maria when she describes him as a Puritan (INSERT QUOTE). In the Elizabethan era, Puritans were stereotypically associated with being kill-joys and an excessive hatred of theatre. Maria is one of Twelfth Night’s characters whose superior intellect seemingly clashes with her social standingShow MoreRelatedElizabethan Poetry Analysis1292 Words   |  6 PagesThroughout my analysis, I will be discussing these different views of women as seen in Shakespeare’s â€Å"Sonnet 130† and his drama, the Twelfth Night, or What You Will. To begin, I want to provide a brief summary of each literary work I will be discussing. Shakespeare’s â€Å"Sonnet 130† is a poem where the speaker describes his mistress and how she does not meet any of society’s beauty standards that are common in other love novels. Regardless of that, the speaker still loves her. Similarly, the Twelfth NightRead MoreThemes Of Social Mobility Through Marriage1655 Words   |  7 PagesThis paper critically analyses the theme of social mobility through marriage in Shakespeare’s play ‘Twelfth Night’. In addition, the paper highlights how different characters in the play got into higher social classes or desired to be in higher social classes through marriage. This paper holds that in a highly stratified society such as that presented in the Shakespeare’s play; marriage plays a significant role in in social class mobility. As opposed to some traditional society where marriage wasRead MoreScene Analysis Of The Twelfth Night1351 Words   |  6 Pages Our group proposed, presented, and directing the stage performance for the Twelfth Night. In the beginning of the semester I had no clue of what to expect from this course, and reading the syllabus made Shakespeare’s Plays seem complex. 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Identify And Briefly Explain Three Func - 1490 Words

A. Identify and briefly explain three functions of religion (9 marks) Marxism believes it acts as the ‘opium for the exploited working class people’. Religion would cushion the pain of oppression and exploitation in unequal societies such as in a capitalist society. It legitimized and maintained the power of the ruling class – helps to maintain the status quo by preventing the less powerful from changing things. Feminists see religion as a conservative force because it acts as an ideology that legitimates patriarchal power and maintains women’s subordination in the family and wider society. Functionalists see religion acting as a ‘collective conscience’. Bringing people to have shared beliefs and moral attitudes which operate as a†¦show more content†¦Neo Marxists, a modernised version of Marxism, holds such a view. Neo-Marxist ‘Otto Maduro’ comments on how religion has the power to spark revolutionary change. He points to the example in Latin America, a predominantly catholic country. During the Somoza regime, many priests began to break away from the Catholic Church, claiming that it was their God-given duty to help and release those who were oppressed. They began cooperating with Marxists, and started to preach â€Å"liberation theology† (movement with strong commitment to poor and opposition to military dictatorships). These religious views challenged the status quo, and led to a revolution in Nicaragua. This example highlights how religion can acts as a force for social change, and there are many other examples which support the claims of supports of this view. Parkin for example, comments on how the Christian Churches of southern America provided an organisational structure for the black â€Å"civil rights movement† during the age of apartheid. Nelson mentions a number of examples of when religion has undermined authority or promoted change; such as when the Catholic Church in Poland opposed Communism, and how Archbishop Desmond Tutu was a strong opponent of apartheid. Perhaps the mostShow MoreRelatedOverview of Hrm93778 Words   |  376 PagesHRM? Explain why are we concerned about HRM? Discuss Road-map of HRM VU Lesson 1 LESSON OVERVIEW This chapter introduces the students with the basic concepts of the human resource management (HRM). During the lecture, we will be discussing the three main things, i.e. the introduction to HRM, the importance of HRM, and a brief discussion of the Resource topics that will follow today’s lecture. A basic concept of management states that manager works in organizations. Organization has three basicRead MoreManaging the International Value Chain in the Automotive Industry60457 Words   |  242 Pagesresource management and infrastructure (Porter 1986a: 29-32).2 This detailed description of the value chain is useful for analyzing âž” competitive advantages. Breaking down a company into its individual value activities makes it possible to identify the current and potential contribution of each activity to the company’s competitive position (Porter 1986a: 19). The value activities of a company, whether they are primary or secondary, can be distr ibuted among different countries. The geographicalRead MoreHsc General Math Textbook with Answers153542 Words   |  615 PagesCambridge HOTmaths lessons, spreadsheet ï ¬ les (Excel format) and PowerPoint ï ¬ les are available to support this textbook. In the electronic version of the textbook (PDF) these icons are hyperlinks to the material in question. Numbers under the icons identify the lesson or ï ¬ le in the teaching program. Cambridge HOTmaths revision material available online with subscription Spreadsheet ï ¬ le available on teacher disk PowerPoint ï ¬ le available on student and teacher disk About the author Greg Powers isRead MoreMonte Carlo Simulation218872 Words   |  876 Pagesdiscuss them explicitly. In addition, an appendix gives precise statements of the most important tools from stochastic calculus. This book divides roughly into three parts. The ï ¬ rst part, Chapters 1–3, develops fundamentals of Monte Carlo methods. Chapter 1 summarizes the theoretical foundations of derivatives pricing and Monte Carlo. It explains the principles by which a pricing problem can be formulated as an integration problem to which Monte Carlo is then applicable. Chapter 2 discusses random number

Complex Formation and Precipitation free essay sample

Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction, or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft amp; Constable, 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution, it considered as precipitate. Commonly, the solid will fall out of the solute phase and sinks to the bottom part of the solution. However, the solid may float on top of the solution or suspended within the solution if the precipitate is less than the aqueous solution. On the other hand, complex formation is the soluble compound that can increase the solubility of an insoluble salt form in aqueos solution (Housecroft amp; Constable, 2006). They are formed from a cation such as water or ammonia that has pair of electrons that become attracted to the positively charged cation. In terms of the solubility, the formation of a complex lowers the concentration of the cation in the solution. In this experiment, there are 3 parts need to be done which is complex formation, weak acids and bases and precipitation reaction. During complex formation experiment, student needs to observe the different reaction occur when adding ammonia or sodium hydroxide in small quantity and in excess. At the second part, student needs to measure the pH of different solution by using universal indicator paper and determine whether each solution is acidic, basic or neutral. Lastly, the precipitation reaction is observed by using phosphates, chlorides and silver halides groups. AIMS The main objective of this experiment was to identify certain inorganic reaction types and the differences in solubility of silver halides. Thus, a series of inorganic reactions was carried out as an introduction to complex formation and precipitation. All the reaction in this experiment involved alteration of equilibrium by changing concentration to make precipitation to form or dissolve. Other than that, weak acid and bases of the solution can be identified and students able to write the balanced equations for inorganic reactions. PRE-LAB QUESTIONS 1. Precipitation reaction is a type of reaction that forms a solid in a solution as a result of chemical reaction or supersaturating a solution. This reaction involves changing the soluble ions into insoluble compound and as a result precipitate is formed when the solution has been saturated by a compound (Heitz, 2005). 2. Inorganic complex consists of a central ion or atom (usually metallic) that is surrounded by anions or molecules bound to the central ion/metal via chemical bonds that range in strength from weak to strong (Heitz, 2005). 3. Trigonal planar, tetrahedral and octahedral. METHODS * PART A: COMPLEX FORMATION (AMMONIA COMPLEXES) . 0. 5 cm3 of dilute zinc nitrate, cupric nitrate and lead nitrate solutions was poured into 3 different test tubes. 2. 4 M of ammonia solution was added dropwise in each test tube until each solution turn alkaline (test with pH paper). 3. Ammonia solution was added more and observes if any precipitate dissolves. 4. The experiment was repeated by re placing the ammonia solution with 2 M of sodium hydroxide. * PART A: COMPLEX FORMATION (IODIDE COMPLEXES) 1. Saturated solution of potassium hydroxide was added dropwise to 0. 5 cm3 of 0. 1 M mercuric nitrate solution until the precipitate of HgI2 just dissolves by forming [HgI4]2-. . Saturated solution of potassium hydroxide was added dropwise to 5 drops of 0. 1 M lead nitrate solution until the precipitate of PbI2 just dissolves by forming [PbI4]2-. 3. The solution of [PbI4]2- was added to about 10 times its volume of distilled water in a medium test tube. 4. The amounts of I- required to dissolve the precipitates formed was compared between Hg (II) and Pb (II). * PART B: WEAK ACIDS AND BASES 1. The pH of distilled water, sodium chloride, aluminium sulphate, ammonium chloride, trisodium phosphate and sodium acetate was measured by using universal indicator paper. 2. Each solution was determined whether it is acidic, basic or neutral. 3. The main ions present in solution and acid-base equation for each solution was recorded. * PART C: PRECIPITATION REACTIONS (PHOSPHATES) 1. 1 cm3 of each of potassium chloride, manganous chloride, magnesium chloride, calcium chloride and cupric sulphate was placed into separate test tubes. 2. 1 cm3 of trisodium phosphate solution was added to each test tube and comment on the possible reasons for the formation of a precipitate. 3. A few drops of 1 M HCl were added to any precipitate formed, shake carefully and any observations were recorded. PART C: PRECIPITATION REACTIONS (CHLORIDES) 1. 1 cm3 of concentrated hydrochloric acid was added to 2 cm3 of saturated sodium chloride solution. 2. The precipitate was allowed to settle before the liquid was pouring off into the mixture and add water. * PART C: PRECIPITATION REACTIONS (SILVER HALIDES) 1. Place 10 drops of sodium chloride, sodium bromide and sodium iodide solut ion into three separate test-tubes. 2. 3 drops of silver nitrate solution was added to each test tube. Then, the precipitate was allowed to settle and pour off the liquid. 3. The solubility of any precipitates was tested in 4 M ammonia solution. . Steps 1 and 2 of this experiment were repeated. 5. The solubility of any precipitated was tested in concentrated ammonia solution (density 0. 880 g cm-3) RESULTS AND DISCUSSION * PART A: COMPLEX FORMATION (AMMONIA COMPLEXES) Table 1: Result of adding ammonia solution to form Ammonia Complex Reactants| Observation| Equation| Zinc nitrate and ammonia solution| * Turn red litmus paper into blue. * White precipitate was formed with cloudy solution. | Zn2+aq+2OH-aq-ZnOH2S| Zinc nitrate and ammonia solution (excess)| * Turn red litmus paper into blue. Clear solution is obtained with all precipitate dissolved in excess ammonia. | Zn(OH)2(S)+4HN3 Zn(NH3)4(aq)2++2OH-aq| Cuprix nitrate and ammonia solution| * Turn red litmus paper into blue. * Blue precipitate was formed. | Cu2+aq+2OH-aq? Cu(OH)2(S)| Cuprix nitrate and ammonia solution (excess)| * Turn red litmus paper into blue. * Clear blue solution is obtained with all precipitate dissolved in excess ammonia. | Cu(OH)2(S)+4HN3Cu(NH3)4(aq)2++2OH-aq| Lead nitrate and ammonia solution| * Turn red litmus paper into blue. * White precipitate was formed with clear solution| Pb2+aq+2OH-aq? Pb(OH)2(S)| Lead nitrate and ammonia solution (excess)| * Turn red litmus paper into blue. * Clear solution is obtained with all precipitate dissolved in excess ammonia. | Pb(OH)2(s) + 4NH3(aq) ? [Pb(NH3)4](aq) + 2OH-(aq)| DISCUSSION| Zinc nitrate, cuprix nitrate and lead nitrate produce white precipitate when reacted with 4 M ammonia and dissolve in excess ammonia solution because they were partially hydrolyzed in water. The solubility of all three precipitate was enhanced by excess ammonia ions although they were insoluble in water. Ammonia acts as ligands where OH group has been replaced with NH3 to form a complex ion. Table 2: Result of adding sodium hydroxide solution to form Ammonia Complex Reactants| Observation| Equation| Zinc nitrate and sodium hydroxide solution| * Turn red litmus paper into blue. * White precipitate was formed with cloudy solution. | Zn(NO3)2aq+2NaOHaqZn(OH)2(S)+2NaNO3aq| Zinc nitrate and sodium hydroxide solution (excess)| * Turn red litmus paper into blu e. * Clear solution is obtained with all precipitate dissolved in excess sodium hydroxide. | Zn(OH)2(aq)+2OH-aqZn(OH)4(aq)2-| Cuprix nitrate and sodium hydroxide solution| * Turn red litmus paper into blue. Blue precipitate was formed with cloudy solution. | CuNO32aq+2NaOHaqCu(OH)2(S)+2NaNO3aq| Cuprix nitrate and sodium hydroxide solution (excess)| * Turn red litmus paper into blue. * Precipitate did not dissolve in excess sodium hydroxide result in dark blue solution. | CuNO32aq+2NaOHaqCu(OH)2(S)+2NaNO3aq| Lead nitrate and sodium hydroxide solution| * Turn red litmus paper into blue. * White precipitate was formed with cloudy solution. | Pb(NO3)2aq+2NaOHaqPb(OH)2(S)+2NaNO3aq| Lead nitrate and sodium hydroxide solution (excess)| * Turn red litmus paper into blue. Clear solution is obtained with all precipitate dissolved in excess sodium hydroxide. | Pb(OH)2(aq)+2OH-aqPb(OH)4(aq)2-| DISCUSSION| The precipitate was formed when sodium hydroxide were reacted with all the three solution and were dissolved when the amount of sodium hydroxide was excess. This shows that the solubility was enhanced by an excess of sodium hydroxide ions as more sodium hydroxide ions can bind with each of the solutions. | * PART A: COMPLEX FORMATION (IODIDE COMPLEXES) Table 3: Results of adding Potassium Iodide (KI) to form Iodide Complex Reactants| Observation| Equation| Mercuric nitrate solution and saturated potassium iodide| * The solution turns to orange colour at the first drop. * The clear solution is obtained after 6 drops of saturated potassium iodide. | * First dropHg2+aq+2I-aq? HgI2(S) * After six dropsHgI2(s) + 2I-(aq) HgI42-(aq)| Lead nitrate solution and saturated potassium iodide| * The solution turns to bright yellow colour at the first drop. * The clear solution is obtained after 15 drops of saturated potassium iodide. * After 10 times of its volume of distilled water (80 ml) was added, the precipitate appeared again| * First dropPb2+aq+2I-aq? PbI2(S) * After fifteen dropsPbI2(S)+2I-aq? PbI42-(aq) * Adding waterPbI42-(aq) + H2O(l) ? PbI2(s) + 2I-(aq)| DISCUSSION| Mercuric nitrate solution shows lower stability constant as compared to lead nitrate solution because only six drops of saturated potassium iodide is needed to dissolve the precipitate formed (Lead nitrate need fifteen drops to dissolve the precipitate). Thus, lead nitrate have higher relative stability constant as compared to the mercuric nitrate solution. | * PART B: WEAK ACID AND BASES Table 4: Reaction, Ions and their Relationship in Weak Acid/Bases Reactants| Observation| Equation| Comment| Distilled water| * pH = 6 * Acidic solution * Main ions present:H+,OH- | * H2Ol ? H3O+aq +OH-aq| * Distilled water supposed to have neutral pH condition which is 7. * The different in the result might due to the presence of the other ions in the distilled water. | Sodium chloride| * pH = 5 * Acidic solution * Main ions present:Na+, Cl-,H+,OH-| * NaClaq ? Na+aq+ Cl-aq| * Sodium chloride supposed to have neutral pH condition because it is neutral salt. * The different in the result might due to the presence of contaminant in the solution used during experiment. Aluminium sulphate| * pH = 2 * Acidic solution * Main ions present:AlH2O62+,SO42-| * AlH2O62+(aq)+H2Oaq? AlH2O3OH(aq)+H+aq| * Due to the presence of H+ ion after dissociation, the solution is acidic and one of the strongest acid as the pH value is lower. | Ammonium chloride| * pH = 5 * Acidic solution * Main ions present:NH4+,Cl-| * NH4+(aq)+H2Ol? H3O+aq+NH3aq| * The pH value shows almost to neutral value as the present H3O+aq r esult to acid properties and NH3aq gave result to basic properties. Trisodium phosphate| * pH = 12 * Basic solution * Main ions present:Na+,PO43-| * HPO42-aq+H2Ol? H2PO4+aq+OH-aq| * Due to the presence of OH- ion after dissociation, the solution is basic and one of the strongest basic as the pH value is higher. | Sodium acetate| * pH = 9 * Basic solution * Main ions present:Na+,CH3COO-| * CH3COO-aq+H2Ol? CH3COOHaq+OH-aq| * Due to the presence of OH- ion after dissociation, the solution has basic properties solution. | * PART C: PRECIPITATION REACTIONS (PHOSPHATES) Table 5: Results of adding trisodium phosphate (Na3PO4) and HCl to different solution. Reactants| Observation| Equation| Potassium chloride and trisodium phosphate solution| * White precipitate were formed | Na3PO4(aq) ? 3Na+(aq) + PO43-(aq)3K+(aq) + PO43-(aq) ? K3PO4(aq)| Potassium chloride, trisodium phosphate and hydrochloric acid| * All precipitate was dissolved and solution is soluble in HCl. | K3PO4S+HCl(aq)? 3KCl(aq)+H3PO4aq| Manganous chloride and trisodium phosphate solution| * White precipitate was formed with cloudy solution. | Na3PO4(aq) ? 3Na+(aq) + PO43-(aq)3Mn2+aq+2PO43-aq? Mn3PO42S| Manganous chloride, trisodium phosphate and hydrochloric acid| * All precipitate was dissolved and solution is soluble in HCl. | Mn3PO42S+6HCl(aq)? 3MnCl2(aq)+2H3PO4aq| Magnesium chloride and trisodium phosphate solution| * White precipitate was formed with cloudy solution. | Na3PO4(aq) ? 3Na+(aq) + PO43-(aq)3Mg2+aq+2PO43-aq? Mg3PO42S| Magnesium chloride, trisodium phosphate and hydrochloric acid| * All precipitate was dissolved and solution is soluble in HCl. | Mg3PO42S+6HCl(aq)? 3MgCl2(aq)+2H3PO4aq| Calcium chloride and trisodium phosphate solution| * White precipitate was formed with cloudy solution. Na3PO4(aq) ? 3Na+(aq) + PO43-(aq)3Ca2+aq+2PO43-aq? Ca3PO42S| Calcium chloride, trisodium phosphate and hydrochloric acid| * All precipitate was dissolved and solution is soluble in HCl. | Ca3PO42S+6HCl(aq)? 3CaCl2(aq)+2H3PO4aq| Cupric sulphate and trisodium phosphate solution| * Blue precipitate was formed with cloudy solution. | 3Cu2+(aq) + 2PO43-(aq) ? Cu3(PO4)2(s)| Cupric sulfate, trisodium phosphate and hydrochloric acid| * All precipitate was dissolved and the solution become soluble (blue in colour)| Cu3(PO4)2(s) + 6HCl(aq) ? 3CuCl2(aq)+ 2 H3PO4(aq)| DISCUSSION| Potassium chloride, manganous chloride, magnesium chloride, calcium chloride and cupric sulphate formed precipitate when reacted with trisodium phosphate solution. All the precipitate then dissolve when hydrochloric acid was added into the mixture to produce metal phosphates and sodium chloride. | * PART C: PRECIPITATION REACTIONS (CHLORIDES) Table 6: Results of adding Concentrated HCl and H2O to saturated NaCl Solution Reactants| Observation| Equation| Potassium chloride and trisodium phosphate solution| * White precipitate were formed | Na+aq+ Cl-aq? NaClsHCl(aq) ? H+(aq) + Cl-(aq)| Potassium chloride, trisodium phosphate solution and water| * White precipitate formed was completely dissolved. | NaCl(s) + H2O(l) ? NaOH(aq) + HCl(aq)| DISCUSSION| The white precipitated was formed because the product, NaCl which is a neutral common salt was white in colour. When water was added, it elimininates the excess Cl- and H+ ions, favoured the backward reaction and thus NaCl is soluble in water. As a result white precipitate dissolved and colourless solution formed. | * PART C: PRECIPITATION REACTIONS (SILVER HALIDES) Table 7: Results of adding AgNO3 and NH3 solution to Sodium Halides Reactants| Observation| Equation| Comment| Sodium chloride and silver nitrate solution| White precipitate was formed with cloudy solution. | AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++Cl-? AgCl (s)| The white precipitate is AgCl because it does not dissolve in water. | Sodium chloride, silver nitrate and ammonia solution| Precipitate dissolved completely to give a colourless solution| AgCl (s)+2NH3(aq)? AgNH32+ (aq)+Cl-(aq)| When AgCl was reacted with ammonia solution, AgNH32+was formed and it was soluble in water as the NH3 ions was able to bind with water molecules. Sodium bromide and silver nitrate solution| Creamy precipitate was formed with cloudy solution. | AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++Br-? Br| AgNH32+is soluble in water as it can bind with water molecules. | Sodium bromide, silver nitrate and ammonia solution| Precipitate was almost unchanged because it did not dissolve completely (partially) in ammonia solutio n| AgBr (s)+2NH3(aq)? AgNH32+ (aq)+Br-(aq)| This precipitate partially dissolves in 4 M ammonia solution. | Sodium iodide and silver nitrate solution| Pale yellow precipitate was formed with cloudy solution. | AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++IAgI (s)| The reaction of NaI with silver nitrate forming a precipitate of AgI| Sodium iodide, silver nitrate and ammonia solution| Precipitate did not dissolve in the mixture of ammonia solution| AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++IAgI (s)| This compound was very insoluble in water, so it will not bind with water molecules, even if reacted with ammonia solution| Table 8: Results of adding AgNO3 and concentrated NH3 solution to Sodium Halides Reactants| Observation| Equation| Comment| Sodium chloride and silver nitrate solution| White precipitate was formed with cloudy solution. | AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++Cl-? AgCl (s)| The white precipitate is AgCl because it does not dissolve in water. | Sodium chloride, silver nitrate and concentratedammonia solution| Precipitate dissolved completely to give a colourless solution| AgCl (s)+2NH3(aq)? AgNH32+ (aq)+Cl-(aq)| When AgCl was reacted with concentrated ammonia solution, AgNH32+was formed and it was soluble in water as the NH3 ions was able to bind with water molecules. | Sodium bromide and silver nitrate solution| Creamy precipitate was formed with cloudy solution. | AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++Br-? Br| AgNH32+is soluble in water as it can bind with water molecules. Sodium bromide, silver nitrate and ammonia solution| Precipitate dissolved completely to give a colourless solution| AgBr (s)+2NH3(aq)? AgNH32+ (aq)+Br-(aq)| By adding concentrated ammonia solution, the precipitate (AgBr) dissolved completely. | Sodium iodide and silver nitrate solution| Pale yellow precipitate was formed with cloudy solution. | AgN O3(aq) ? Ag+(aq) + NO3-(aq) Ag++IAgI (s)| The reaction of NaI with silver nitrate forming a precipitate of AgI| Sodium iodide, silver nitrate and ammonia solution| Precipitate did not dissolve in the mixture of ammonia solution| AgNO3(aq) ? Ag+(aq) + NO3-(aq) Ag++IAgI (s)| Adding either diluted or concentrated NH3 solution, did not make the precipitate (AgI) became soluble because it will not dissolve. Thus, it can be said that solubility of silver halides decreases down the group. | QUESTIONS 1. The relative stability constants of iodide complex of Hg (II) is less than the iodide complex of Pb(II). This is because from the result obtained, only 6 drops of iodide were required to dissolve the precipitates formed by the mercuric nitrate, Hg (II) as compared to lead nitrate, Pb(II) that required 15 drops to dissolve the precipitate. Thus, iodide complex of Pb(II) is more stable than iodide complex of Hg(II) because more drops of iodide were required to dissolve lead nitrate, Pb(II) than mercuric nitrate, Hg(II). 2. Commonly, using a pH meter and an indicator paper during the experiment would result in different pH value obtained. This is because pH meter is more precise in giving pH values up to 2 decimal places while indicator paper only gives an approximation of pH based on colour with reference to chart. Thus, due to difficulty to differentiate the colours observed as referred to chart, indicator paper is not the best method to determine the accurate pH value of the mixture. 3. Equation of the reaction: NaCl Na+ + Cl- The precipitate formed was sodium salt crystal (NaCl). According to Le Chatelier’s principle, this change in reaction acts to counteract the increase of Cl- concentration (Silberberg, 2006). When concentrated HCl was added, concentration of chloride ion (Cl) increases. Thus, equilibrium will shift to the left. Therefore, reverse reaction was favoured result in more solid salt precipitate (NaCl) was formed. 4. In the case of silver halides, the chloride is the most soluble in ammonia and the iodide is the least while for the case of calcium halides the reverse trend is seen. This is due to the solubility of the group 2 sulphates which decreased down the trend. Thus, silver and metal halides were soluble in ammonia as they formed complex ions which were soluble. CONCLUSION In conclusion, the complex formation and precipitation reactions were able to establish thus met the aims of this experiment. Thus, it can be concluded that ammonia and hydroxide ion can act as a Lewis base since a complex ion was formed when a metal cation is covalently bonded to ligands. Other than that, weak acid and base will dissociates partially in water while strong acid and base dissociate completely in water. Finally, the formation of the precipitate (product) can be controlled by controlling the pH of the reaction. REFERENCES Heitz. , M(2005) General Chemistry: An Integrated Approach, Chapter 16: More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions, 4th Edition, Prentice Hall, Inc. , State University of New York. pp. 715-718 Housecroft, C. E. amp; Constable, E. C. (2006), Introduction to spectroscopy, in Chemistry, 3rd Edition, Pearson Education, England. pp. 951-970 Silberberg, M. S. (2006), Chemistry: The Molecular Nature of Matter and Change, 4th Edition, Mc Graw Hill International Edition, New York, pp. 1013-1019.

The Point of No Return free essay sample

John Adams, one of the American Revolutions central figures, recalled in his later writings that Americans were committed to independence in their hearts long before war broke out in America in 1775. This suggests that American independence was inevitable; however, this was not the case. Just twelve year earlier in 1 763, Americans cheerfully celebrated the British victory in the Seven Years War, taking great pleasure in their identity as Britons and jealously guarding their much-celebrated rights which they believed they possessed by virtue of membership in what they saw as the worlds greatest empire.Seeing this, few would have predicted that by 1776, a revolution would be developing in British America. On the surface, the recipe for discontent seemed lacking. There was no economic crisis among the colonies; in fact, they were relatively prosperous. Yet, how did everything change in just a few short years? What occurred to make the American colonists set aside their differences, and unanimously declare their independence? Actually a lot happened between 1 763 and 1776. We will write a custom essay sample on The Point of No Return or any similar topic specifically for you Do Not WasteYour Time HIRE WRITER Only 13.90 / page The events that occurred during these important years created sharp divisions among he English, among the colonists, and between the English and the Colonists. On the surface, the colonists believed they were unfairly taxed, watched over like children, and ignored when they attempted to address grievances. On the other side, the British found the colonists unwilling to pay their fair share for the administration of the Empire. After all, the English paid more in taxes than was asked of any American during the whole period of crisis. Most historians believe that the American Revolution occurred in three major phases. They refer to the first phase the Imperial Crisis. The Imperial Crisis was the intellectual and political conflict over the constitutional relationship between Britain and the thirteen American colonies. It began with Parliaments passage of the Stamp Act in 1765 imposing a stamp tax on printed documents, such as, newspapers, contracts, and licenses throughout the American colonies.Other acts that led to crisis in the first phase were the Declaratory Act, the Townsend Acts, the Boston Massacre, the Sugar Act, the Tea Act, and the Boston Tea Party. The second phase was the Revolutionary War itself, which began in 1775, when constitutional debate led o bloodshed between the Americans and British at Lexington and Concord, in Massachusetts. General Thomas Gage, the British garrison in Boston knew that the townspeople had been procuring arms, ammunition and training to be able to fight on a minutes notice. However, he believed his army was too small and decided to await reinforcements. Officers tried to convince Gage that Americans would not fight and would actually retreat before any show of force by Britain. Gage resisted the officers and continued to resist when orders came over from England to arrest American rebels, John Hancock and Sam Adams. It was believed that the two were in the vicinity of Lexington. It was only when Gage learned that the Americans had stored a vast supply of gun powder in Concord, which was only eighteen miles outside of Boston that he decided to take action.On April 18, 1 775, Gage deployed a detachment of approximately 1 ,OHO soldiers from Boston on the road to Lexington and Concord. A surprise attack was his intention, but Patriots in Boston were at watch of the British movements. During the night, William Dates and Paul Revere made that historical ride out to warn the villages and farms. When the British troops arrived the next day, they were met by several dozen minutemen and the first shots The shots heard round the world had been fired. The final phase is most often referred to as the Critical Period.This was a time when American leaders faced the new problems of preserving the liberty and independence. It was in this phase of the conflict that made the war truly revolutionary -? not only because it introduced a new kind of combat, but also because it had the effect of monopolizing and politicking large groups of the population who had previously remained aloof from the trudge. In conclusion, the American Revolution was the American peoples defense of their right not to be deprived of their property without their consent.The Stamp Act Crisis was the first of several battles in that defense. It has been argued over time that the point of no return, that specific time in history when relations between the American colonists and the British became so bad that there was no chance Of a reconciliation ever occurring, was the Stamp Act Crisis. Other historians believe it was the shots fired at Lexington or the Boston Tea Party. However, the colonists had already been defied by the Royal Proclamation of 1763.