buffers are effective and provide opportunity for the use of the Henderson-Hasselbalch equation to prepare a buffer of a specific pH. Three different buffer systems were initially investigated; volumes of weak acid and weak bases of specified concentration were prepared and titrated against strong acid or strong base solutions with pH readings taken at frequent intervals to determine pH ranges over which the systems are most effective. The Henderson-Hasselbalch equation was used to calculate an appropriate
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a negative charge and if pH < pI‚ the protein will have a positive charge. Buffer I has a pH >5‚ meaning both proteins carry a negative charge and bind to the DEAE (a positively charged resin). (b) pH = pKa + log10(Base/Acid) [Base = mM of sodium acetate; Acid = mM of acetic acid] = 4.7 + log10 (40/40) = 4.7 In order for the catalase to elute from the column‚ it must have lost its negative charge and stopped binding to the DEAE. Lowering the pH nullifies the negative charge on the protein
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of indicators and instrumental detection of equivalence points in acid-base titration. Objective 1. To understand the importance of choosing suitable indicators for detecting the end points of acid-base titrations. 2. To obtain titration curves for some acid-base titrations. Materials and Method (Please refer to the General Chemistry BPH2012 practical manual pg 4-5) Results Part I: Suitability of Indicators A.Strong acid-weak base titration 1 2 Initial Burette Reading (mL) 19.50
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Chemistry Practice Exam and Notes Effective Fall 2013 About the College Board® The College Board is a mission-driven not-for-profit organization that connects students to college success and opportunity. Founded in 1900‚ the College Board was created to expand access to higher education. Today‚ the membership association is made up of over 6‚000 of the world’s leading educational institutions and is dedicated to promoting excellence and equity in education. Each year‚ the College
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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 acetic acid? (there may be more than one correct answer) a
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|Acid and Base Ionization Constants | | | |Acid Ionization Constant (Ka) - the equilibrium constant for a weak acid. | |Acid Ionization Constants
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shows that the buffer systems made with sodium acetate and acetic acid were effect when titrated with the strong acid and the strong base. Comparison of all the solutions shows that the concepts of buffers holds true for the results from the experimentation. Introduction The main objective of this lab was to test the ability of buffered and unbuffered solutions to resist changes in pH with the addition of strong acids and strong acid. This will be accomplished by making two sets of five different
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determine the rate constants‚ k1‚ for the methyl acetate hydrolysis reaction at 25 °C and 35 °C‚ as well as the overall activation energy of the reaction. Methods Methyl acetate was placed in an HCl solution‚ in which it reacts with water to form acetic acid over time. At each time interval‚ an aliquot of the mixture was removed for titration against NaOH to determine the concentration of the acetic acid produced. From the amount of acetic acid produced overtime‚ the rate constant‚ k1‚ can be determined
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Study guide for exam 3 Chem 1212 Fall 2014 (chapters 3‚4‚ 14‚15) Chapter 3 Nomenclature ionic compounds‚ molecular compounds‚ simple organic compounds‚ hydrates‚ acids Know the names and charges of the polyatomic ions Calculation molecular weight mw Molar mass of compound Number particles = NA x n Mass % Determination of empirical formula and molecular formula Combustion analysis Balancing equations Chapter 4 Limiting reactant Mole to mole conversion from reaction stoichiometry Theoretical yield
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geological samples. Acid hydrolysis of Nb/Ta samples separates Indium from major matrix elements like Nb and Ta and the remaining elements do not influence the selective extraction and preconcentration of In and its subsequent determination by ICP-AES or flame AAS. The silica rich geological samples are decomposed by HF-H2SO4-HCl treatment followed by dissolution in 6M HCl before applying solvent extraction procedure. In Nb/Ta type of samples‚ Indium was separated from Nb and Ta by acid hydrolysis‚ involving
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