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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equilibrium constant reversibility LeChâtelier’s Principle ICE table Q and Keq major species minor species Keq‚f vs Keq‚r rate constant vs. equilibrium expressions significance of magnitude of Keq equilibrium shift with concentration changes equilibrium shift with temperature changes equilibrium shift with volume changes Chapter 16: Acid-Base Euilibrium Brønsted-Lowry acid Brønsted-Lowry base amphoteric water equilibrium constant pH pOH pH
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solubility product constant (Thorne‚ 90). This constant is important because it does not change at a given temperature‚ regardless of the solution a compound is in; a smaller constant would indicate lower overall solubility. It is important to note that comparing the Ksp values of two or more compounds can only be done if the compounds share the same dissociation stoichiometry. In this experiment‚ 1 mol of Ca(OH)2 is used to produce 3 mol of products. In order to compare this constant to another compound
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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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50M KI and 0.010M Na2S2O3 and 2.5 cm3 of starch solution into the second boiling tube. Place another thermometer in this solution and stand it in the water bath. 4.> When the temperatures of the two solutions are equal and constant (to within ± 1℃)‚ pour the contents of the second boiling tube into the first‚ shake to mix‚ and start the stop-watch. 5.>
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Ka1 Ka2) (approx.) (eq 13-4) |Example: Calculate the hydronium ion concentration of a 0.100 M NaHCO3 solution. | |We first examine the assumptions leading to Equation 13-4. The dissociation constants for H2CO3 are Ka1 = 1.5e-4 and Ka2 = | |4.69e-11. | |[H3O+] = ((1.5e-4 x 4.69e-11) = 8.4e-8 M
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defined as the quantity of strong acid or base that must be added to change the pH of one liter of solution by one pH unit. The buffer range is the pH range where a buffer effectively neutralizes added acids and bases‚ while maintaining a relatively constant pH. To effectively maintain a pH range‚ a buffer must consist of a weak conjugate acid-base pair‚ meaning either a. a weak acid and its conjugate base‚ or b. a weak base and its conjugate acid. The use of one or the other will simply depend upon
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stronger base than H20‚ equilibrium lies to left. HX is a weak acid -In every acid-base reaction‚ equilibrium favors transfer of the proton from the stronger acid to the stronger base to form the weaker acid and the weaker base. -Kc (equilibrium constant) 1 (right) Know that water auto-ionizes into hydrogen ions and hydroxide ions‚ expressed by Kw‚ the ion product of water. - Kw=[H3O+][OH-] -
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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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