Chemistry Virtual Textbook

Acid-base chemistry can be extremely confusing, particularly when dealing with weak acids and bases. This set of lessons presents an updated view of the Brønsted-Lowry theory that makes it easy to understand answers to common questions: What's the fundamental difference between a strong acid and a weak acid? Can acid A neutralize base B? Why are some salts acidic and others alkaline? How do buffers work? What governs the shapes of titration curves? This complete rewrite of the previous 1996 pdf document is now organized into seven lessons covering all aspects of the subject. Much emphasis is placed on the practical aspects of calculations, including how to deal with quadratic equations and how to judge when approximations are appropriate.

Advanced Level Inorganic Chemistry Revision UK GCE AS A2 A Level Notes doc brown iphone ipad notepad notebook netbook [ORGANIC NOTES] * [INORGANIC NOTES] * [PHYSICAL-THEORETICAL NOTES] * A Level QUESTIONS UK Exam syllabuses AQA Advanced Subsidiary GCE AS Level Chemistry and AQA GCE A2 Advanced A Level Chemistry EDEXCEL GCE Advanced Subsidiary AS Level Chemistry & EDEXCEL GCE Advanced A Level A2 Chemistry OCR GCE Advanced Subsidiary AS Level Chemistry (NOT Salters) and OCR GCE A Level A2 Chemistry (NOT Salters) Salters Advanced Subsidiary AS Level Chemistry SALTERS & Salters Advanced A Level A2 Chemistry SALTERS WJEC Advanced Subsidiary AS GCE Chemistry and WJEC Advanced A2 GCE Chemistry CCEA Advanced Subsidiary AS GCE Chemistry and CEA-CCEA Advanced A2 GCE Chemistry Cambridge pre-U GCE chemistry * Cambridge International Examinations (CIE) GCE 9701 Chemistry ALL Website content copyright © Dr Phil Brown 2000-2014 All rights reserved on revision notes, images, puzzles, quizzes, worksheets, x-words etc. * Copying of website material is not permitted * chemhelp@tiscali.co.uk

level Chemistry Chemical Equilibria Revision - Chemical Equilibria A reversible reaction is one where there is a forward and backward reaction occurring: The double arrow signifies a reversible reaction. If in the above reaction the concentrations of A, B, C, D do not change, although the reaction is still in progress, then the forward rate must equal the backward rate. A situation known as dynamic equilibrium has been reached. Any dynamic equilibrium can be described in terms of its equilibrium constant, Kc. The equilibrium constant is the product of the molar concentrations of the products raised to the power of its coefficient in the stoichiometric equation, divided by the product of molar concentrations of the reactants, each raised to the power of its coefficient in the stoichiometric equation. So for the reaction: The equilibrium constant is given by: Where [] represents the concentration of the species in moldm-3. For gaseous systems, we use Kp instead of Kc.

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