Physics H7ABC Welcome to the archival Web page for U.C. Berkeley’s Physics H7ABC‚ Honors Physics for Scientists and Engineers‚ Fall 1998‚ Spring 1999‚ and Fall 1999. Instructor: (Prof.) Mark Strovink. I have a research web page‚ a standardized U.C. Berkeley web page‚ and a statement of research interests. Physics H7A (Mechanics and Vibrations) Problem set solutions initially composed by E.A. ("Ted") Baltz Graduate Student Instructors: David Bacon and Elizabeth Wu Physics H7B (Electromagnetism
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Diploma Programme Chemistry data booklet First examinations 2009 Diploma Programme Chemistry data booklet First published March 2007 Revised edition published September 2008 International Baccalaureate Peterson House‚ Malthouse Avenue‚ Cardiff Gate Cardiff‚ Wales GB CF23 8GL United Kingdom Phone: +44 29 2054 7777 Fax: +44 29 2054 7778 Website: http://www.ibo.org © International Baccalaureate Organization 2008 The International Baccalaureate (IB) offers three high quality and
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Chapter 1: Introduction 1 Introduction E-learning is the delivery of training and learning using means of electronic media‚ such as computers‚ Internet or intranet (Tastle‚ White‚ & Shackleton‚ 2005). Three basic ingredients of e-learning constitute: content and instructional methods; ways of delivering content and methods; and achievement of personal and organisational goals. These ingredients are also referred as the what‚ how and why elements of e-learning respectively (Clark & Mayer‚ 2008)
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Experiments 4A-C: Synthesis and Component Analysis of an Iron (III) Oxalate Complex My Name TA‚ Section B## Work Performed on 10/23‚ 10/30‚ & 11/4‚ 200# Report due Tuesday‚ November ##‚ 200# 1. Abstract This experiment initially involved the synthesis of an iron (III) oxalate complex with the general formula Kw[Fex(C2O4)y]·zH2O. The variables x‚ y‚ and z were determined through the duration of the entire experiment. From 1.2000g of Fe(NH4)2(SO4)2 were synthesized 1.1###g of K3[FeIII(C2O4)3]·3H2O
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CH 125 INORGANIC CHEMISTRY FOR MICROBIOLOGY Laboratory Manual 2013 Edition By Brian Clark‚ Marco Castillo & Patrick Chan CENTENNIAL COLLEGE OF APPLIED ARTS & TECHNOLOGY‚ SCARBOROUGH‚ ONTARIO Preliminary Laboratory Information - CH 125 The following safety information is provided to the student in order to ensure that all students and college staff working in the laboratory are aware of common industrial laboratory safety practices. Laboratory
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Chemistry Stage 3 Standards Guide Exemplification of Standards through the 2010 WACE Examination Chemistry: Stage 3 Standards Guide 1 2010/33606 Copyright © Curriculum Council‚ 2011 This document—apart from any third party copyright material contained in it—may be freely copied‚ or communicated on an intranet‚ for noncommercial purposes by educational institutions‚ provided that it is not changed in any way and that the Curriculum Council is acknowledged as the copyright owner. Copying
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know the elements of life – and how the reduction and oxidative of some of these drive bioenergetics oxidize carbon (i.e. glucose source) and reduce oxygen (electron acceptor) (CHNOPS) and iron (Fe; trace element; Fe also important to obtain cellular energy). Nutrition: CHNOPS Trace Elements: Iron (Fe)‚ Ni‚ Mg‚ Mo‚ Mn‚ Ca (important in humans due to osteoblastic activity)‚ Co Occupancy: beat out others for a spot to live‚ e.g. microbiota (normal flora) Resistance: defend against microbes‚ eukaryotes
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Pneumonia Case Study NUR 213 Gina Perry‚ SN2 Central Maine Community College Abstract This paper illustrates how the student nurse cared for a patient with pneumonia. The student nurse was assigned a patient on a medical surgical unit during clinical rotation. During this time‚ the student nurse observed and interacted with the patient‚ conducted a full head to toe assessment as well as routine scheduled assessments‚ administered medications‚ and created a plan of care. A brief description of
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parents. This is the intellectual forerunner of the tabula rasa that Locke learned from Ibn Tufail. Hb(k/LT02goUXVTUsUyTUVFUP U6RwRPQ__c FHTc2eXBrV‚kMbLvv/LSCsfffq9J ---jf7zbrup@‚mu 6Qucy Gm7046l18cckihhIg5xfob4ekabi2)kft‚9kaEJ6MVVyVVI‚mWlPW vm))Sn1 9amtrtuvlp4Wggs5KvSmnzmM.AXq/vYO0mezyNk5/ B Yroc3g‚Z0LoLGli)2.QStqt‚YgjrvgjlRlcxEt sl3TtcwY5Y8 BP/OnMOEQJV8ChOFu3 ORyMVDq-9R i0(Of ymslLRPL/xxHHZ3fPxYESw.1RdxihPXRUjyRCW4nZcadUjV_pFWN_ymJHnYJjA _mJtzj5a56zVwxWkEnbGwOEjtol mR6HpowpZAPHyu-mG1cu5W(dNyLkQgCtL_pbKGpHoeWtMjs
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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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