ASSIGMNET 1 | Research on student difficulties in Understanding Chemical reactions | Misconceptions on Strength of Acids and Bases | | Mariyam Zaina‚ 015482 | | | TITLE & INTRODUCTION Title: Misconceptions on Strength of Acids and Bases Researches shows that students often develops new theories about how the natural world works‚ prior to formal science education and frequently those theories are different to those of scientists(Demircioğlu et al.‚ 2005). Students develop
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ACIDS AND BASES The reason that acid-base reactions are so important is that many of the things you come into contact with on a daily basis are either acids or bases. Most fruits are acids‚ as are carbonated beverages‚ tea‚ and battery acid. Common household bases include baking soda‚ ammonia‚ soap‚ and antacids. What are acids and bases? There are not one but three common definitions used to describe acids and bases: 1. Arrhenius acids and bases 2. Brønsted-Lowry acids and bases 3. Lewis acids
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Worksheet - Acids‚ Bases and Salts 1. I am pure water. When heated my pH (increases‚ decreases)‚ because more of my water molecules dissociate. 2. I am a 0.020 M solution of weak acid‚ HA. If I only dissociate to the extent of 1.50%‚ what is the value of my Ka? 3. I am a 0.20 M solution of hydrocyanic acid‚ HCN‚ with a Ka of 4.93 x 10¯ 10 . What is my pH? 4. I am a buffer made from 0.10 M acetic acid and 0.15 M sodium acetate. If the Ka for acetic acid is 1.77 x 10¯ 5 ‚ what is my pH? 5. I am
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University of the Philippines‚ Diliman‚ Quezon City‚ Philippines Date Due: September 20‚ 2013 Date Submitted: September 20‚ 2013 RESULTS AND DISCUSSION An experiment was conducted to determine the purity of Hydrogen Phthalate sample and its dissociation constant. To perform the experiment with the utmost precision‚ equivalence point was determined using potentiometric determination. Two methods exist for potentiometric determination exist: direct and indirect. Potentiometric techniques are often
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-1A2 CHEMISTRY MODULE 4 definitions (aqa) Rate of Reaction The rate of change of concentration with time (mathematically d[X]/dt). Units are mol.dm-3.s-1 (moles per cubic decimetre per second) Initial Rate This is the rate at the very beginning of the reaction when all the starting concentrations are known exactly. Rate Equation Rate Expression A mathematical expression which relates the rate to the concentrations of substances involved in the reaction Rate Constant‚ k This is the multiplying
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The dissociation of protons from oxalic acid proceeds in a stepwise manner as for other polyprotic acids. Loss of a single proton 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
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The ionic product of water = Kw = [H+] x [OH‐] = 1.0 x 10‐14 mol2 dm‐6 at 298 K The expression varies with temperature pH + pOH = 14 Ka x Kb = 1.0 x 10‐14 pKa + pKb = 14 Acids The Ka is the acid dissociation constant and is a measure of the strength of an acid or in other words a measure of the ability of an acid to dissociate into ions Complete the table and statements below Ka pKa 1 x 10‐3 9.4 ‐5 1 x 10
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Bronsted-Lowry- Acid is a proton donor and a base a proton acceptor * Lewis- An acid is an electron pair acceptor‚ and I base is an electron pair donor * Conjugate base & acids * Ka= [products]/[reactants] * Acid dissociation constant * 14.2 Acid Strength * In a strong acid dissociate almost 100% * Ka is large * Strong acid yields weak conjugate base * Weak Acid * Does not dissociate much * The weaker the acid
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De Leon‚ Jo-Anna Maria N. 3ChEA Group No. 2 Experiment No. 5 Spectrophotometric Determination of pKa I. Introduction The equilibrium constant of the dissociation of an indicator in water will be determined experimentally using spectroscopic method.This experiment aims to demonstrate the principle of equilibrium and the interaction of matter with light. II. Methodology Figure . UV-VIS Spectrophotometer 10 solutions covering the entire pH range from 1 to 13 were prepared
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strength. proton base2 + proton acid2 For example‚ perchloric and hydrochloric acids are strong acids in water. If anhydrous acetic acid‚ a weaker proton acceptor than water‚ is substituted as the solvent‚ neither of these acids undergoes complete dissociation Many solvents are proton donors or proton acceptors and can thus induce basic or acidic behavior in solutes dissolved in them. For example‚ in an aqueous solution of ammonia‚ water can Acetic acid acts as a differentiating solvent toward donate
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