Stephen G. Abelada BS ChE IV Date Submitted: January 4‚ 2012 ChE 171 Assignment 1. Essential and Non-essential Amino acids Amino acids are organic compounds which contain both an amino group and a carboxyl group and may be divided into two groups basing on whether they are produced internally by the human body or not: essential and non-essential amino acids (hyperphysics.phy-astr.gsu.edu‚ 2012). An essential amino acid (indispensable amino acid) is an amino
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BRONSTED-LOWRY ACIDS AND BASES 1. The Bronsted-Lowry definition There are many definitions of acids and bases in existence‚ but the most useful one is the Bronsted-Lowry definition: An acid is a substance which can behave as a proton (re presented as a hydrogen ion‚ H+) donor. Any substance which contains hydrogen bonded to a more electronegative element can thus behave as an acid: HCl == H+ + Cl- H2SO4 == H+ + HSO4- A base is a substance which can behave as a proton acceptor. Any
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ANSWERS TO QUESTIONS: 1. a. in distilled water: Cu(OH)2(s) (( Cu2+(aq) + 2OH-(aq) Ksp Cu(OH)2 Keq = Ksp Cu(OH)2 = 2.2 x 10-20 b. + 6.0M H2C2O4 Cu(OH)2(s) (( Cu2+(aq) + 2OH-(aq) Ksp Cu(OH)2 H2C2O4 (( H+ + HC2O4- Ka1 H2C2O4 HC2O4- (( H+ + C2O42- Ka2 H2C2O4 Cu2+ + C2O42- (( CuC2O4 1/Ksp CuC2O4 2(OH- + H+ (( H2O) 1/K2w Net Keq = (Ksp Cu(OH)2 x Ka1 x Ka2 )/Ksp CuC2O4
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Acids And BAses Acids And BAses 8.1 8.2 8.3 8.4 18.1 18.2 18.3 18.4 18.5 Theories of acids and bases Properties of acids and bases Strong and weak acids & bases The pH scale Calculations involving acids and bases (AHL) Buffer solutions (AHL) Salt hydrolysis (AHL) Acid-base titrations (AHL) Indicators (AHL) 8 8.1 THeORies OF Acids And BAses 8.1.1 Define acids and bases according to the Brønsted–Lowry and Lewis theories. 8.1.2 Deduce whether or not a species could act as a Brønsted–Lowry
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AbstractWater is important substance for all living organisms. The physical and chemical properties of water play a central role in biological structure and function of the organism. The ionization ability of water to form H+ and OH- ions make it very unique. The hydrogen-ion concentration of biological system is usually preferred as the pH system‚ which determines the pH level of dilute aqueous solutions. In this laboratory‚ the data collected from the experiment will be used to graph the titration
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The relationship between Ka and pKa is that Ka is the equilibrium constant for the dissociation of a weak acid and pKa is the half-equivalence point where pH=pKa. In addition to the pH‚ Ka is an indication of an acids strength; pKa = - log Ka. B. The potential sources for errors in this experiment are the inconsistent and miscounting
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amounts of water. References: [1] Mohrig‚ J. R.; Hammond‚ C. N.; Morrill‚ T. C.; Neckers‚ D. C. 1998 Experimental Organic Chemistry‚ New York: Freeman‚ pp. 32-36. [2] www.chemblink.com II. Potentiometric Determination of the Purity and Acid Dissociation Constant of Salicylic Acid Purpose: Part II of the experiment utilizes the concept of potentiometric titration in the determination of the pKa‚ a measure of the relative acidity of an acid‚ of the salicylic acid product in Part I. Potentiometric
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NAME_________________________________ STAMP________________ PERIOD____ PICTURES & GRAPHS A. The Atom 1. Calculate the average atomic mass using the spectrum below. 2. Answer the questions regarding the energy level diagram shown. a) The emission lines for the series above are in the IR‚ Vis and UV regions. Match the series with the region and justify your choice (FYI – AP you do not need to memorize the names of the series. IB will need to know then for next year). b) Would the wavelength
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CROATICA CHEMICA ACTA CCACAA 78 (1) 99¿103 (2005) ISSN-0011-1643 CCA-2984 Original Scientific Paper Acid Value Determination in Vegetable Oils by Indirect Titration in Aqueous-alcohol Media Elena Kardash* and Yakov I. Tur’yan National Physical Laboratory of Israel (INPL)‚ Givat Ram‚ Jerusalem 91904‚ Israel RECEIVED JANUARY 16‚ 2004; REVISED JULY 21‚ 2004; ACCEPTED OCTOBER 28‚ 2004 Keywords acid value vegetable oils indirect titration A new method of acid value determination in
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Chemistry102 5/7/2013 Lecture Presentation Chapter 17 Additional Aspects of Aqueous Equilibria John D. Bookstaver St. Charles Community College Cottleville‚ MO © 2012 Pearson Education‚ Inc. Common Ion Effect HA(aq) + H2O(l) ⇔ A−(aq) + H3O+(aq) • Adding a salt containing the anion NaA‚ which • is the conjugate base of the acid (the common ion)‚ shifts the position of equilibrium to the left This causes the pH to be higher than the pH of the acid solution 9lowering the H3O+ ion concentration
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