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Na2c2h3o2 Essay

Words: 1292, Paragraphs: 2, Pages: 5

Paper type: Essay

This essay sample on Na2c2h3o2 provides all necessary basic information on this matter, including the most common “for and against” arguments. Below are the introduction, body and conclusion parts of this essay.

The purpose of this experiment is to become familiar with precipitation reactions. According to the textbook, precipitation is the process where a chemical reaction leads to the formation of a solid, which is called a “precipitate.” These types of chemical reactions are called precipitation reactions. To understand the formation of a solid in a chemical reaction, it is important to understand the key components that yield the precipitate.Precipitation reactions specifically occur when aqueous solutions of ionic solutes are mixed to produce a solid. The term “aqueous” refers to the state of the substance, showing that it dissolves in water. When a solid containing ions dissolves in water, the ions separate and move around independently. When two aqueous solutions are mixed, the solution becomes a mixed solution -one that contains independent ions. To determine what solid, if any, is formed, it is necessary to predict the result using the rules of solubility. Solubility is a solid’s ability to dissolve in water.A soluble solid will readily dissolve in water, whereas an insoluble solid will not dissolve, or change in ways so small that they are not visible to the naked eye. By knowing the solubility rules of ionic compounds, it is possible to know whether a precipitate will form in a reaction, and what the precipitate is.Methods and MaterialsThis experiment required the mixture of several different substances, followed by observation of the results. To perform these tests, a microtiter plate was used to contain the individual drops of substances. The substances provided included the following solutes: sulfuric acid, hydrochloric acid, silver nitrate, sodium carbonate, sodium chloride, potassium chromate, lead acetate, sodium sulfate, and barium chloride.Using pipets, these solutes were carefully mixed on the microtiter plate, which was used as a reaction chamber. Carefully, the reagents were dispersed and mixed, while the reactions observed and recorded. To discover the results of the reactions, it was necessary to use solubility rules to predict the reactions. The order of the reactions as well as the results can be seen in Data Table 1.Results and ObservationsTable 1. Reactants and PrecipitatesReactantReactantBalanced EquationPrecipitateSilver Nitrate – AgNO3Sodium Chloride – NaClAgNO3(aq) + NaCl(aq) –> AgCl(s) + NaNO3(aq)AgClSilver Nitrate – AgNO3Hydrochloric Acid – HClHCl(aq) + AgNO3(aq) –>HNO3(aq) +AgCl(s)AgClSilver Nitrate – AgNO3Sulfuric Acid – H2SO4AgNO3(aq) + H2SO4(aq) –>Ag2SO4(s) + HNO3(aq)Ag2SO4Silver Nitrate – AgNO3Sodium Sulfate – Na2SO42AgNO3(aq) + Na2SO4(aq) –> Ag2SO4(s) + 2NaNO3(aq)Ag2SO4Silver Nitrate – AgNO3Sodium Carbonate – Na2CO32AgNO3(aq) + Na2CO3(aq) –> Ag2CO3(s) + 2NaNO3(aq)Ag2CO3Silver Nitrate – AgNO3Potassium Carbonate – K2CO32AgNO3(aq) + K2CO3(aq) –> Ag2CO3(s) + 2KNO3(aq)Ag2CO3Silver Nitrate – AgNO3Lead(II)Acetate – Pb(C2H3O2)2AgNO3(aq) + Pb(C2H3O2)2(aq) –> Ag(C2H3O2)2(aq) + Pb(NO3)2(aq)No PrecipitateSilver Nitrate – AgNO3Barium Chloride – BaCl22AgNO3(aq) + BaCl2(aq) –> 2AgCl(s) + Ba(NO3)2(aq)AgClPotassium Carbonate – K2CO3Lead(II)Acetate – Pb(C2H3O2)2K2CO3(aq) + Pb(C2H3O2)2(aq) –> K2(C2H3O2)2(aq) + PbCO3(s)PbCO3Potassium Carbonate – K2CO3Barium Chloride – BaCl2K2CO3(aq) + BaCl2(aq) –> KCl2(aq) + BaCO3(s)BaCO3Potassium Carbonate – K2CO3Copper(II)Sulfate – CuSO4K2CO3(aq) + CuSO4(aq) –>K2SO4(aq) + CuCO3(s)CuCO3Lead(II)Acetate – Pb(C2H3O2)2Sodium Carbonate – Na2CO3Pb(C2H3O2)2(aq) + Na2CO3(aq) –> PbCO3(s) + Na2(C2H3O2)2(aq)PbCO3Lead(II)Acetate – Pb(C2H3O2)2Sodium Chloride – NaClPb(C2H3O2)2(aq) + NaCl(aq) –> PbCl2(aq) + Na2(C2H3O2)2(aq)No PrecipitateLead(II)Acetate – Pb(C2H3O2)2Sodium Sulfate – Na2SO4Pb(C2H3O2)2(aq) + Na2SO4(aq) –> PbSO4(s) + Na2(C2H3O2)2(aq)PbSO4Lead(II)Acetate – Pb(C2H3O2)2Sulfuric Acid – H2SO4Pb(C2H3O2)2(aq) + H2SO4(aq) –> PbSO4(s) + H2(C2H3O2)2(aq)PbSO4Lead(II)Acetate – Pb(C2H3O2)2Barium Chloride – BaCl2Pb(C2H3O2)2(aq) + BaCl2(aq) –> PbCl2(aq) + Ba(C2H3O2)2(aq)No PrecipitateLead(II)Acetate – Pb(C2H3O2)2Hydrochloric Acid – HClPb(C2H3O2)2(aq) + HCl(aq) –> PbCl2(aq) + H2(C2H3O2)2(aq)No PrecipitateLead(II)Acetate – Pb(C2H3O2)2Copper(II)Sulfate – CuSO4Pb(C2H3O2)2(aq) + CuSO4(aq) –> PbSO4(s) + Cu(C2H3O2)2(aq)PbSO4Barium Chloride – BaCl2Sodium Carbonate – Na2CO3BaCl2(aq) + Na2CO3(aq) –> BaCO3(s) + NaCl(aq)BaCO3Barium Chloride – BaCl2Sodium Sulfate – Na2SO4BaCl2(aq) + Na2SO4(aq) –> BaSO4(s) + NaCl(aq)BaSO4Barium Chloride – BaCl2Sulfuric Acid – H2SO4BaCl2(aq) + H2SO4(aq) –> BaSO4(s) + HCl(aq)BaSO4Barium Chloride – BaCl2Copper(II)Sulfate – CuSO4BaCl2(aq) + CuSO4(aq) –> BaSO4(s) + CuCl(aq)BaSO4Sodium Chloride – NaClSodium Carbonate – Na2CO3NaCl(aq) + Na2CO3(aq) –> Na2CO3(aq) + NaCl(aq)No PrecipitateAmmonium Chloride – NH4ClLead(II)Acetate – Pb(C2H3O2)2NH4Cl(aq) + Pb(C2H3O2)2(aq) –> NH4(C2H3O2)2(aq) + PbCl2(aq)No PrecipitateAmmonium Chloride – NH4ClSilver Nitrate – AgNO3NH4Cl(aq) + AgNO3(aq) –> NH4NO3(aq) + AgCl(s)AgClAmmonium Chloride – NH4ClCopper(II)Sulfate – CuSO4NH4Cl(aq) + CuSO4(aq) –> NH4SO4(aq) + CuCl(aq)No PrecipitateTable 2. Net Ionic Equations and ObservationsReactantsNet Ionic EquationObservationsAgNO3, NaClAg+(aq) + Cl-(aq) –> AgCl(s)drops turned cloudy-whiteAgNO3, HClCl-(aq) + Ag-(aq) –> AgCl(s)drops turned cloudy-whiteAgNO3, H2SO4Ag+(aq) + Ag+(aq) + SO4-(aq) –>Ag2SO4(s)developed soft-white particlesAgNO3, Na2SO4Ag+(aq) + Ag+(aq) + SO4-(aq) –> Ag2SO4(s)developed yellow tintAgNO3, Na2CO3Ag+(aq) + Ag+(aq) + CO3-(aq) –> Ag2CO3(s)translucent cloudy-white and yellow particlesAgNO3, K2CO3Ag+(aq) + Ag+(aq) + CO3-(aq) –> Ag2CO3(s)reddish-brown color changeAgNO3, Pb(C2H3O2)2No precipitate formed.no apparent changeAgNO3, BaCl2Ag+(aq) + Ag+(aq) + Cl-(aq) + Cl-(aq) –> 2AgCl(s)developed thick cloudy-white colorK2CO3, Pb(C2H3O2)2CO3-(aq) + Pb-(aq) –> PbCO3(s)developed white particles in yellow liquidK2CO3, BaCl2CO3-(aq) + Ba+(aq) –> BaCO3(s)solid/cloudy yellow liquidK2CO3, CuSO4CO3-(aq) + Cu+(aq) –> CuCO3(s)developed white particles in yellow liquidPb(C2H3O2)2, Na2CO3Pb+(aq) + CO3-(aq) –> PbCO3(s)turned misty/foggy whitePb(C2H3O2)2, NaClNo precipitate formed.no apparent changePb(C2H3O2)2, Na2SO4Pb+(aq) + SO4-(aq) –> PbSO4(s)turned cloudy-whitePb(C2H3O2)2, H2SO4Pb+(aq) + SO4-(aq) –> PbSO4(s)changed into soft-white colorPb(C2H3O2)2, BaCl2No precipitate formed.no apparent changePb(C2H3O2)2, HClNo precipitate formed.no apparent changePb(C2H3O2)2, CuSO4Pb+(aq) + SO4-(aq) –> PbSO4(s)developed soft-white colorBaCl2, Na2CO3Ba+(aq) + CO3-(aq) –> BaCO3(s)white precipitation on clear liquidBaCl2, Na2SO4Ba+(aq) + SO4-(aq) –> BaSO4(s)- – – – (wasn’t in class/not recorded)BaCl2, H2SO4Ba+(aq) + SO4-(aq) –> BaSO4(s)- – – – (wasn’t in class/not recorded)BaCl2, CuSO4Ba+(aq) + SO4-(aq) –> BaSO4(s)- – – – (wasn’t in class/not recorded)NaCl, Na2CO3No precipitate formed.no apparent changeNH4Cl, Pb(C2H3O2)2No precipitate formed.no apparent changeNH4Cl, AgNO3Cl-(aq) + Ag+(aq) –> AgCl(s)- – – – (wasn’t in class/not recorded)NH4Cl, CuSO4No precipitate formed.no apparent changeDiscussionIn this lab, it was made clear, through numerous chemical reactions, what exactly occurs in a precipitation reaction. The standard definition reads that a precipitation reaction occurs when a solid is formed as a result of the mixture of aqueous ions, which sounds obscure. However, the experimentation with many different types of substances shows how consistent and predictable these results can be. Using solubility rules, it is easy to determine whether a precipitate will form, and even know what the solid is.For example, the compound Silver Nitrate, or AgNO3, combined with HCl, or hydrochloric acid, forms the precipitate AgCl, or Silver Chloride. This is known because the solubility rules states that NO3 salts are soluble, as well as chloride salts. However, in the case of AgCl, chloride is not soluble. As soon as this information is attained, it is determined that AgCl is the precipitate, since the remaining ions H and NO3 dissolve in water.QuestionsThe solubility rules used to predict the identity of the precipitates formed in the reactions of this experiment are general “rules of thumb” that hold true in most instances. However, the specific quantity of an ionic solid that will dissolve in a given quantity of solvent is governed by the solubility or the solubility product of the ionic substance. Use your textbook or encyclopedia for each of these terms.Solubility – solubility is physical property of a substance having the ability to dissolve in water.Solubility product – solubility product constants are used to describe saturated solutions of ionic compounds of relatively low solubility. A saturated solution is in a state of dynamic equilibrium between the dissolved, dissociated, ionic compound and the undissolved solid.Source: www.chem.purdue.edu/ConclusionThough chemistry is a very complex science, experimenting with chemical reactions offers a chance to experience and understand the consistent workings of the study. On paper, it seems as though the hundreds of elements and thousands of compound combinations are an endless wall of difficult formulas. Through experiences like these experiments, however, I can firsthand witness the consistency in chemical change, and see exactly how the world functions. Precipitation opened up a new aspect of chemistry -the ability to see and know how ions react in water, and how they react with each other to form new solids. Seeing and understanding why chemical changes happen transforms an endless wall of “dry” formulas into a fascinating world of actual substances found in reality.

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