Hydroxo Compounds in 0.5 - 14 M Naoh Solutions
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Practical Course in General and Inorganic Chemistry III
Practical course in general and inorganic chemistry III. Common acid-base theories The Arrhenius definition - Dissociation of strong/weak acids and bases - Preparation of salts - The limitations of the Arrhenius acid-base theory The Brønsted-Lowry definition - Relative strengths of Brønsted-Lowry acids and bases - Amphiprotic species (the amphoterism) - Types of acid-base reactions - Structures of different boric acids and borax - Preparation of normal salts - Acid salts The Arrhenius acid-base theory (1884) • Acid : dissociate in aqueous solution form hydrogen + or the later-termed oxonium (H 3O ) ions univalent, strong acid: univalent, weak acid: diprotic, strong acid: diprotic, weak acid: triprotic, weak acid: • Stepwise acid dissociation : 1 Relative strength of inorganic oxoacids (Pauling) − + + Om X(OH) n Om+1X(OH) n−1 H acid anhydride m = 3 very strong acid m = 2 strong acid m = 1 weak acid m = 0 very weak acid Arrhenius-bases and anhydrides • Base : in aqueous solution form hydroxide (OH −) ion(s) and cation(s) univalent, strong base: divalent, strong base: univalent, weak base: divalent, weak base: trivalent, weak base: • Base anhydrides = metal-oxides : derived from the base by subtracting the molecules of water • base anhydrides of strong bases: 2 Preparation of salts (Arrhenius) base + acid = salt + water • Preparation of salt from a strong base: • Preparation of salt from a weak base : • If the acid is partially neutralized: acid salt The limitations of the Arrhenius acid-base theory • Although ammonia is well-known as a -
In This Section and in the Next Section on Redox Chemistry, We Will Often Draw on Fundamental Thermodynamic Concepts
Prerequisites for Section III (1-2 weeks) • In this section and in the next section on redox chemistry, we will often draw on fundamental thermodynamic concepts. You should recall the meaning of ∆H, ∆S, and ∆G for chemical and physical changes — and try to think about systems using these concepts. • ∆G˚ = –RTln Keq This relationship is central to relating chemical thermodynamics and equilibrium. • ∆G = ∆H – T∆S for a process with a specified T and P • The above two relationships can be combined to provide invaluable guidance in understanding how a chemist can manipulate ∆H or ∆S (say, by making changes in ∆S˚/R –∆H˚/RT solvents or molecular substituents) to dramatically shift equilibria: Keq = e e . At room temperature, RT ≈ 2.5 kJ/mol, so this equation means that, for example, a change in solvent that causes ∆H to shift by only ~ 6 kJ/mol will shift the equilibrium constant for a reaction by a factor of 10 (roughly). Acids and Bases a. Brønsted Acidity — aqueous equilibria, solvent leveling, periodic trends, oxoacids, anhydrous acids and bases, amphoterism, polyoxo ions, nonaqueous solvents • Brønsted acid = proton donor, Brønsted base = proton acceptor + • pH = –log[H ], pKa = –logKa; pKb = –logKb • [H+][H+] = 10–14 in aqueous solutions • pKa + pKb = 14 – for any conjugate acid-base pair in dilute aqueous solution • recall concepts of conjugate acids and bases; strong acids have weak conjugate bases, weak acids have strong conjugate bases • Things that affect acidity and basicity of organic acids and bases: the ability of a conjugate base (acid) to delocalize negative (positive) charge through inductive effects or resonance affects the strength of an acid (base). -
Final Program
1 General Information SCOPE OF THE CONFERENCE The 11th Joint MMM/Intermag Conference is sponsored jointly by the American Institute of Physics (PCI) and the Magnetics Society of the IEEE, in cooperation with The American Physical Society. Members of the inter- national scientific and engineering communities interested in recent devel- opments in fundamental and applied magnetism are invited to attend the Conference and contribute to its technical sessions. Sessions will include invited and contributed papers, oral and poster presentations and invited symposia. This Conference provides an outstanding opportunity for partici- pants to meet their colleagues and discuss new, advanced and controversial developments. WASHINGTON, DC The 2010 Joint Conference will be held in the nation’s capital. The city wel- comes 15 million visitors each year of which 1.2 million are international. There are more than 100 restaurants located in the downtown area alone, and the city has been called “one of the most exciting restaurant cities on the East Coast” by Travel & Leisure. To obtain an in-depth and current view of what to see and do while you are here, visit the official website at: http://www.washington.org. Here you will find information on how to trav- el to the Marriott Washington Wardman Park from any of the three local air- ports; you can check on the weather in mid-January, and can request a free Visitors Guide prior to making your trip. VISA REQUIREMENTS The US has updated its visa policies to increase security, so it may take you 3-6 months to apply for and receive your visa. -
Inorganic Chemistry for Dummies® Published by John Wiley & Sons, Inc
Inorganic Chemistry Inorganic Chemistry by Michael L. Matson and Alvin W. Orbaek Inorganic Chemistry For Dummies® Published by John Wiley & Sons, Inc. 111 River St. Hoboken, NJ 07030-5774 www.wiley.com Copyright © 2013 by John Wiley & Sons, Inc., Hoboken, New Jersey Published by John Wiley & Sons, Inc., Hoboken, New Jersey Published simultaneously in Canada No part of this publication may be reproduced, stored in a retrieval system or transmitted in any form or by any means, electronic, mechanical, photocopying, recording, scanning or otherwise, except as permitted under Sections 107 or 108 of the 1976 United States Copyright Act, without either the prior written permis- sion of the Publisher, or authorization through payment of the appropriate per-copy fee to the Copyright Clearance Center, 222 Rosewood Drive, Danvers, MA 01923, (978) 750-8400, fax (978) 646-8600. Requests to the Publisher for permission should be addressed to the Permissions Department, John Wiley & Sons, Inc., 111 River Street, Hoboken, NJ 07030, (201) 748-6011, fax (201) 748-6008, or online at http://www.wiley. com/go/permissions. Trademarks: Wiley, the Wiley logo, For Dummies, the Dummies Man logo, A Reference for the Rest of Us!, The Dummies Way, Dummies Daily, The Fun and Easy Way, Dummies.com, Making Everything Easier, and related trade dress are trademarks or registered trademarks of John Wiley & Sons, Inc. and/or its affiliates in the United States and other countries, and may not be used without written permission. All other trade- marks are the property of their respective owners. John Wiley & Sons, Inc., is not associated with any product or vendor mentioned in this book. -
Water Splitting by Heterogeneous Catalysis
!"#$ #"%"" &' () * ( +# ,% - . ( (.( ( . %/ .0! 1 ( % 2 3 . 4 . 5 % . . % . . . . . . 3 % !# 3 ( 3 ( 3 ( 3 %/. . - % . (. 6 7 % ( 2!0! . (/ (3 . 7 % ( ( 3 % . 3 ( %/ . 8 9 3 8 % ( :;0 9 . <= 3 9 . % ( . ( 3 > % !"#$ ?@@ %% @ A B ?? ? ? #;C#C# ,8D$CD#$$D$":D! ,8D$CD#$$D$";"C ! " # $ (#" D# WATER SPLITTING BY HETEROGENEOUS CATALYSIS Henrik Svengren Water splitting by heterogeneous catalysis Henrik Svengren ©Henrik Svengren, Stockholm University 2017 ISBN print 978-91-7797-039-2 ISBN PDF 978-91-7797-040-8 Printed in Sweden by Universitetsservice US-AB, Stockholm 2017 Distributed by the Department of Materials and Environmental Chemistry To my beloved family Cover image + Heterogeneous catalysis of water oxidation according to 2H2O ĺ O2 + 4H on CoSbO4/CoSb2O6, investigated in Paper II. The figure is composed of SEM- and TEM images, structural drawings, reactant- and product molecules. i Examination Faculty opponent Docent Tomas Edvinsson Solid State Physics Department of Engineering Sciences Uppsala University, -
A Review of the Structural Architecture of Tellurium Oxycompounds
Mineralogical Magazine, May 2016, Vol. 80(3), pp. 415–545 REVIEW OPEN ACCESS A review of the structural architecture of tellurium oxycompounds 1 2,* 3 A. G. CHRISTY ,S.J.MILLS AND A. R. KAMPF 1 Research School of Earth Sciences and Department of Applied Mathematics, Research School of Physics and Engineering, Australian National University, Canberra, ACT 2601, Australia 2 Geosciences, Museum Victoria, GPO Box 666, Melbourne, Victoria 3001, Australia 3 Mineral Sciences Department, Natural History Museum of Los Angeles County, 900 Exposition Boulevard, Los Angeles, CA 90007, USA [Received 24 November 2015; Accepted 23 February 2016; Associate Editor: Mark Welch] ABSTRACT Relative to its extremely low abundance in the Earth’s crust, tellurium is the most mineralogically diverse chemical element, with over 160 mineral species known that contain essential Te, many of them with unique crystal structures. We review the crystal structures of 703 tellurium oxysalts for which good refinements exist, including 55 that are known to occur as minerals. The dataset is restricted to compounds where oxygen is the only ligand that is strongly bound to Te, but most of the Periodic Table is represented in the compounds that are reviewed. The dataset contains 375 structures that contain only Te4+ cations and 302 with only Te6+, with 26 of the compounds containing Te in both valence states. Te6+ was almost exclusively in rather regular octahedral coordination by oxygen ligands, with only two instances each of 4- and 5-coordination. Conversely, the lone-pair cation Te4+ displayed irregular coordination, with a broad range of coordination numbers and bond distances. -
General Chemistry/Properties and Theories of Acids and Bases 1 General Chemistry/Properties and Theories of Acids and Bases
General Chemistry/Properties and Theories of Acids and Bases 1 General Chemistry/Properties and Theories of Acids and Bases Acid-Base Reaction Theories Acids and bases are everywhere. Some foods contain acid, like the citric acid in lemons and the lactic acid in dairy. Cleaning products like bleach and ammonia are bases. Chemicals that are acidic or basic are an important part of chemistry. Helpful Hint! You may need to refresh your memory on naming acids. Several different theories explain what composes an acid and a base. The first scientific definition of an acid was proposed by the French chemist Antoine Lavoisier in the eighteenth century. He proposed that acids contained oxygen, although he did not know the dual composition of acids such as hydrochloric acid (HCl). Over the years, much more accurate definitions of acids and bases have been created. Arrhenius Theory The Swedish chemist Svante Arrhenius published his theory of acids and bases in 1887. It can be simply explained by these two points: Arrhenius Acids and Bases 1. An acid is a substance which dissociates in water to produce one or more hydrogen ions (H+). 2. A base is a substance which dissociates in water to produce one or more hydroxide ions (OH-). Based on this definition, you can see that Arrhenius acids must be soluble in water. Arrhenius acid-base reactions can be summarized with three generic equations: Svante Arrhenius General Chemistry/Properties and Theories of Acids and Bases 2 An acid will dissociate in water producing hydrogen ions. A base (usually containing a metal) will dissociate in water to product hydroxide ions. -
Complex Ions and Amphoterism
Chemistry 112: Reactions Involving Complex Ions Page 27 COMPLEX IONS AND AMPHOTERISM his experiment involves the separation and identification of ions using Ttwo important reaction types: (i) the formation of complex ions and (ii) the amphoteric behavior of some metal hydroxides. You have already encoun- tered complex ion formation in the analysis of the silver group ions and in the experiment on metal sulfides, but more needs to be said about this topic as an introduction to this experiment. THE FORMATION OF COMPLEX IONS Although we usually write cation formulas in solution as if they were simple ions, such as Al3+, these ions are actually bound to a number of water mol- ecules arranged around the central ion (see figure below). The water molecules in this case are examples of a much larger class of molecules and ions called ligands that form coordinate covalent bonds with a central metal cation. That is, the bond is of the form L: → Mn+, where L has donated δ+ an otherwise unused lone pair of electrons H As noted in the experiment on the to the electron accepting metal ion. In the 3+ δ+ H O Al silver group ions, a ligand is a Lewis water molecule, there are two lone pairs of •• base (a donor of one or more pairs of electrons on the O atom, and either of these δ− electrons), and the metal ion in the may form a coordinate covalent bond with a complex ion is a Lewis acid (an elec- metal cation. Ligands are often small, polar tron pair acceptor). -
Complex Ions and Amphoterism
Chemistry 112: Reactions Involving Complex Ions Page 27 COMPLEX IONS AND AMPHOTERISM his experiment involves the separation and identification of ions using Ttwo important reaction types: (i) the formation of complex ions and (ii) the amphoteric behavior of some metal hydroxides. You have already encoun- tered complex ion formation in the analysis of the silver group ions and in the experiment on metal sulfides, but more needs to be said about this topic as an introduction to this experiment. THE FORMATION OF COMPLEX IONS Although we usually write cation formulas in solution as if they were simple ions, such as Al3+, these ions are actually bound to a number of water mol- ecules arranged around the central ion (see figure below). The water molecules in this case are examples of a much larger class of molecules and ions called ligands that form coordinate covalent bonds with a central metal cation. That is, the bond is of the form L: → Mn+, where L has donated δ+ an otherwise unused lone pair of electrons H As noted in the experiment on the to the electron accepting metal ion. In the 3+ δ+ H O Al silver group ions, a ligand is a Lewis water molecule, there are two lone pairs of •• base (a donor of one or more pairs of electrons on the O atom, and either of these δ− electrons), and the metal ion in the may form a coordinate covalent bond with a complex ion is a Lewis acid (an elec- metal cation. Ligands are often small, polar tron pair acceptor). -
Articles That May Namic Light Scattering Measurements Related the Upper Freez- Account for Cloud Glaciation at Moderate Supercooling
Atmos. Chem. Phys., 20, 3291–3315, 2020 https://doi.org/10.5194/acp-20-3291-2020 © Author(s) 2020. This work is distributed under the Creative Commons Attribution 4.0 License. Protein aggregates nucleate ice: the example of apoferritin María Cascajo-Castresana1,2,3, Robert O. David3,4, Maiara A. Iriarte-Alonso2, Alexander M. Bittner2,5, and Claudia Marcolli3 1División de Salud, TECNALIA, Parque Tecnológico, Paseo de Mikeletegi, 2, 20009 Donostia, Spain 2CIC nanoGUNE, Tolosa Hiribidea, 76, 20018 Donostia, Spain 3Department of Environmental System Sciences, Institute for Atmospheric and Climate Science, ETH Zurich, 8092 Zurich, Switzerland 4Department of Geosciences, University of Oslo, Oslo, 0315, Norway 5Ikerbasque, Basque Foundation for Science, Ma Díaz de Haro 3, 48013 Bilbao, Spain Correspondence: Claudia Marcolli ([email protected]) Received: 24 September 2019 – Discussion started: 7 October 2019 Revised: 10 February 2020 – Accepted: 17 February 2020 – Published: 20 March 2020 Abstract. Biological material has gained increasing atten- −4 to −11 ◦C and a lower one from −11 to −21 ◦C. Dy- tion recently as a source of ice-nucleating particles that may namic light scattering measurements related the upper freez- account for cloud glaciation at moderate supercooling. While ing range to ice-nucleating sites residing on aggregates and the ice-nucleation (IN) ability of some bacteria can be related the lower freezing range to sites located on misfolded cage to membrane-bound proteins with epitaxial fit to ice, little is monomers or oligomers. The sites proved to persist during known about the IN-active entities present in biological ma- several freeze–thaw cycles performed with the same sam- terial in general. -
Buffer Solution Adapted from WIKI
技 术 资 料 集 锦 NO：20140924 Buffer solution in Biology adapted from WIKI A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an aqueous solution consisting Acids and bases of a mixture of a weak acid and its conjugate base, or vice versa. Its pH changes very little when a small amount ofstrong acid or base is added to it and thus it is used to prevent changes 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. pH Acid–base reaction Contents Acid–base titration Acid-base extraction Dissociation constant 1 Principles of buffering Acid dissociation constant 2 Applications Acid strength o 2.1 Simple buffering agents Acidity function o 2.2 "Universal" buffer mixtures Buffer solutions o 2.3 Common buffer compounds used in biology Proton affinity 3 Buffer capacity Self-ionization of water 4 Calculating buffer pH Amphoterism o 4.1 Monoprotic acids Acid types o 4.2 Polyprotic acids 5 See also Brønsted 6 References Lewis 7 External links Mineral 0510 81819585 | 189 51576701 | QQ: 2642 166682 | [email protected] 1 无锡天演生物技术有限公司 | 江苏省无锡市智慧路 33 号 7 栋 601 室 技 术 资 料 集 锦 NO：20140924 Organic Strong Superacids Principles of buffering Weak Simulated titration of an acidified solution of a weak acid (pKa = Base types 4.7) with alkali. -
Acid Base Equilibrium Pretest
Name: ________________________ Class: ___________________ Date: __________ ID: A Acid Base Equilibrium PreTest Multiple Choice Identify the choice that best completes the statement or answers the question. 1. If a reaction is reversible, what are the relative amounts of reactant and product at the end of the reaction? a. no reactant; all product b. no product; all reactant c. some product; some reactant d. The relationship between reactants and products cannot be determined. 2. What happens to a reaction at equilibrium when more reactant is added to the system? a. The reaction makes more products. b. The reaction makes more reactants. c. The reaction is unchanged. d. The answer cannot be determined. 3. Which of the changes listed below would shift the following reaction to the right? 4HCl(g) + O2 (g) 2Cl2 (g) + 2H2 O(g) a. addition of Cl2 b. removal of O2 c. increase of pressure d. decrease of pressure 4. What is the effect of adding more water to the following equilibrium reaction? CO2 + H2 O H2 CO3 a. More H2 CO3 is produced. b. CO2 concentration increases. c. The equilibrium is pushed in the direction of reactants. d. There is no effect. 8 5. In an equilibrium reaction with a Keq of 1 10 , the ____. a. reactants are favored b. reaction is spontaneous c. the products are favored d. reaction is exothermic 7 6. The Keq of a reaction is 4 10 . At equilibrium, the ____. a. reactants are favored b. products are favored c. reactants and products are present in equal amounts d. rate of the forward reaction is much greater than the rate of the reverse reaction 7.