Honors Chemistry was always a pleasantly productive period. A typical class block entailed only a lesson and worksheet; for example‚ I would speed through a stoichiometry worksheet‚ ensure that I understood limiting reagents‚ and find myself with half of the period to occupy. Some days I would finish homework for other classes‚ while other days I would browse scientific journals on my phone. Occasionally I would use this time to “do math‚” which‚ for someone without much of a background in the subject
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Analysis of Soda Ash and Carbonate-Bicarbonate Mixture Submitted: February 27‚ 2013 Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas España‚ Manila Abstract A standard acid solution like HCl can be used as titrant for the analysis of both soda ash and a carbonate-bicarbonate mixture. In the analysis of soda ash‚ the volume needed to neutralize the soda ash is used to compute for its alkalinity‚ in this experiment we obtained a 17.6 % alkalinity with an error
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__________. A) all chemical reactions have ceased B) the rate constants of the forward and reverse reactions are equal C) the rates of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed 2) Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (s) + H2O (l) ⇌ H3O+ (aq) + F- (aq) A) [HF][H2O] / [H3O+][F-] B) 1 /[HF] C) [H3O+][F-] / [HF][H2O]
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concepts investigated in this lab are insolubility‚ double replacement‚ and limiting reactants. Insolubility occurs when a solute is incapable of dissolving in a solvent. A double replacement occurs when both of the compounds’ cations are exchanged. Lastly‚ limiting reactants are factors that limit and determine the amount of product produced. All of these concepts come together to
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Chemistry Investigation 14: ------------------------------------------------- To determine the enthalpy change of reaction for: ------------------------------------------------- Na2CO3(aq) + H2O(l) + CO2(g) → 2NaHCO3(aq) Given: S1— Anhydrous sodium carbonate (Na2CO3) S2— Anhydrous sodium hydrogen carbonate (NaHCO3) A1—Aqueous sulfuric acid (H2SO4)‚ 0.500mol dm-3 Apparatus | Uncertainty | Measuring cylinder | ± 0.5 ml | Electronic Balance | ± 0.001 g | Data logger | ±0.2 ℃ |
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Acids & Bases: Reactions‚ Standardizations‚ & Titrations Experiments 21 & 22 Experimental Overview: The procedure for this experiment was carried out as instructed in the laboratory manual‚ Experiments in General Chemistry‚ 4th ed.‚ S.L. Murov‚ Experiment 21‚ Acids and Bases: Reactions and Standardizations‚ and Experiment 22‚ Acids and Bases: Analysis. There were modifications made by the instructor to dilute the 6M NaOH to 0.1M in 300mls
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of a mole of iron and copper. The result obtained in this lab usually have less than a one percent error. Fe(s) + CuSO4 (aq) > FeSO4(aq) + Cu(s) Iron powder cupric sulfate ferrous sulfate copper In the reaction‚ iron will be the limiting reagent; it will be completely used up in the reaction. Cupric sulfate will be in excess; not all of it will be used up in the reaction. The number of moles of iron that react will equal the number of moles of copper produced. The reaction indicates the
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Experiment 5 Title: Volumetric Analysis – stoichiometry Purpose: To determine the exact concentration of a monobasic acid‚ HX (KA1) Materials and apparatus: 1. Volumetric flask and stopper (250cm3) 2. Electric balance ±0.01 g 3. Pipette and pipette filler (25cm3) 4. Volumetric flask and stopper (100cm3) 5. Burettes (50cm3) 6. Retort stand and clamp 7. White tile 8. Wash bottle filled with distilled water 9. Spatula 10. Titration
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Introduction On a general level‚ alkenes can be formed from the dehydration of an alcohol in the presence of a strong acid. The acid simply acts as a catalyst and as such increases the reaction time but while doing so does not affect the overall stoichiometry. The usual mole ratio of such reaction is therefore 1:1 which means that the theoretical yield of Alkene in mole is equal to the amount of alcohol used in the reaction. Below are the reaction and the overall
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Synthesis of 3-methyl-3-heptanol In this experiment‚ an example of an organometallic compound which has a carbon magnesium bond will be utilized to form a tertiary alcohol. Grignard reagents have been extremely useful in the synthesis of a large number of classes of organic functional groups. Although Grignard reagents are unstable and decompose in air and moisture‚ they can be prepared and used immediately with moderate difficulty in the undergraduate organic chemistry laboratory. Care will need
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