March 17‚ 2013 March 17‚ 2013 Name : Ryan annasdass arokiasamy ID : 1206875 Group Members : Chan Pei Qie‚Chong Ven Yen Name : Ryan annasdass arokiasamy ID : 1206875 Group Members : Chan Pei Qie‚Chong Ven Yen experiment 19 kinetics : the study of a chemical reaction experiment 19 kinetics : the study of a chemical reaction Results Part A [I-] / mol dm-3 | [S2O82-] / mol dm-3 | [S2O32-] / mol dm-3 | Time /s | Rate of I2 formation / mol dm-3 s-1 | 0.2 | 0.2 | 0.01 | 1.25 | 0
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Ngoc Pham Chem162B Lab #2: Trends in Periodic Table Date: 01/10/2011 Lab partner: Ian Bauer Result Section: Table I: The solubility of the alkaline earth metal ions | SO42- | CO32- | C2O42- | IO32- | Mg2+ | S | I | S | S | Ca2+ | I | S | S | I | Sr2+ | S | S | S | I | Ba2+ | I | I | I | S | Key: I- insoluble‚ S-soluble Table II: Color of water (Halide) and Halogen (Hexane) layers | Cl2 | Br2 | I2 | Hexane layer | Clear | orange | Pink | Water layer | Clear‚
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of strong acid or base is added to it and thus it is used to prevent any change in the pH of a solution. Buffer solutions are used as a means of keeping pH at a nearly constant value in a wide variety of chemical applications. Many life forms thrive only in a relatively small pH range so they utilize a buffer solution to maintain a constant pH. One example of a buffer solution found in nature is blood. So far in discussing pH we have dealt only with solutions obtained by adding a single acid‚ such as
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act as the proton acceptor. An acid (HA) reacts with a base (in this case H2O) to form the conjugate base of the acid (A-) and the conjugate acid of the base (H3O+). HA + H2O H 3O + + A - The equilibrium constant for an acid-base reaction is expressed as a dissociation constant (Kd )‚ with the concentrations of the reactants in the denominator and the concentrations of the products in the numerator. Kd = [ H3O+][A-] [HA][ H2O] Most organic acids are weak. They do not ionize (dissociate)
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results in the monovalent hydrogenoxalate anion HC2O4−. A salt with this anion is sometimes called an acid oxalate‚ monobasic oxalate‚ or hydrogen oxalate. The equilibrium constant (Ka) for loss of the first proton is 5.37×10−2 (pKa = 1.27). The loss of the second proton‚ which yields the oxalate ion has an equilibrium constant of 5.25×10−5 (pKa = 4.28). These values imply that‚ in solutions with neutral pH‚ there is no oxalic acid‚ and only trace amounts of hydrogen oxalate.[1] The literature is
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Homework 1_Key BCH2333 Winter 2015 Topics covered: review‚ Chemical Evolution‚ Water‚ Non-covalent bonds‚ Acid/base‚ pH 1. i) Convert using scientific notation to liters: 4 nanoliters‚ 4 x 10-9 L‚ 20 microliters‚ 2x10-5 L‚ 35 milliliters‚ 3.5 x 10-2 L‚ 10 deciliters‚ 1 L‚ 7 kiloliters 7 x 103 L ii) Convert using scientific notation to grams: 6 mg‚ 6 x 10-3 g‚ 21 µg‚ 2.1 x 10-5 g‚ 503 ng‚ 5.03 x 10-7 g‚ 10 kg‚ 1 x 104 g 2. Which of the following properties of water explains its ability to dissolve
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acid to donate a proton. • The more readily a compound donates a proton‚ the stronger an acid it is. • Acidity is measured by an equilibrium constant. • When a Brønsted-Lowry acid H—A is dissolved in water‚ an acid-base reaction occurs‚ and an equilibrium constant can be written for the reaction. Because the concentration of the solvent H2O is essentially constant‚ the equation can be rearranged and a new
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Experiment Martin Novick Group 14‚ Chemical Engineering Laboratory Submitted to Prof. David B. Henthorn September 25‚ 2012 Summary The goal of this project was to determine the pre-exponential factor‚ k o ‚ the activation energy‚ E‚ and the reaction rate constants‚ k‚ of the saponification process of ethyl acetate using sodium hydroxide (NaOH) at 5 temperature between 15 and 25 degrees Celsius. Two trails were performed at temperatures 16‚ 18‚ 20‚ 22‚ and 24 degrees Celsius. The main equipment of the project
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with each other and with the walls of the container. Due to these collisions the speeds and the kinetic energies of the individual molecules keep on changing. However at a given temperature‚ the average kinetic energy of the gas molecules remains constant. If at a given temperature‚ n1 molecules have speed v1‚ n2 molecules have speed v2‚ n3 molecules have speed v3‚ and so on. Then‚ the total kinetic energy (EK) of the gas at this temperature is given by where m is the mass of the molecule.
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triphenyl phosphate and tetrabutylammonium benzoate for that of benzyl benzoate. Their interfacial concentrations were a unique function of the concentrations of tetrabutylammonium bromide and the respective sodium salts. The intrinsic reaction rate constants‚ for the synthetic reactions of triphenyl phosphate and benzyl benzoate‚ which were evaluated by fitting the rate data to the model prediction‚ were 2.33 X lo6 and 2.56 m3/kmol-s at 303 K‚ respectively. Introduction Phase-transfer catalyst can enhance
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