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Acids and bases pdf file: >> http://zuu.cloudz.pw/download?file=acids+and+bases+pdf+file << (Download)
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Introduction to acid-base chemistry. A Chem1 Reference Text. Stephen K. Lower. Simon Fraser University. Contents. 1 Acids. 2. 1.1 Acids and the hydrogen ion . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2. 2 Bases. 3. 3 Neutralization. 4. 4 Dissociation of water. 4. 5 The pH scale. 5. 6 Titration. 6. 6.1 Titration curves .
Acids neutralize bases in a neutralization reaction. An acid and a base combine to make a salt and water. A salt is any ionic compound that could be made with the anion of an acid and the cation of a base. The hydrogen ion of the acid and the hydroxide ion of the base unite to form water. Acids corrode active metals.
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).
The Water or Arrhenius Theory was widely accepted up to the early years of this century. It defines an acid as a hydrogen compound ionizing in water to give hydrogen ions, and a base as a hy<iToxyl compound which gives hydroxide ions in water. The neutralization reaction between an acid and a base produces a salt
bases - H+ acceptors. Lewis Acids & Lewis Bases. ? more broad way to define acids and bases. ? Lewis acids – electron pair acceptors metal cations (Mn+) and boron are common. Lewis acids species that are electron deficient; electrophiles. ? Lewis bases – electron pair donors species with O, N, halogen frequently
Acid Base Chemistry. 4.1. Terminology: 4.1.1. Bronsted / Lowry Acid: "An acid is a substance which can donate a hydrogen ion (H+) or a proton, while a base is a substance that accepts a proton. B- + HA <---> HB + A- base1 + acid1 <---> acid2 + base 2. Where HB = the conjugate acid. A- = the conjugate base. Examples:
Chapter 4. Acids and bases. Bronsted acidity 111. 4.1 Proton transfer equilibria in water 112. 4.2 Solvent levelling 119. 4.3 The solvent system de_nition of acids and bases 121. Characteristics of Bronsted acids 122. 4.4 Periodic trends in aqua acid strength 122. 4.5 Simple oxoacids 123. 4.6 Anhydrous oxides 126.
acids and bases ionize completely, but weak acids and bases ionize only partially. 18.3 Hydrogen Ions and pH. MAIN Idea pH and pOH are logarithmic scales that express the concentrations of hydrogen ions and hydroxide ions in aqueous solutions. 18.4 Neutralization. MAIN Idea In a neutralization reaction, an acid reacts
Chapter 16: Acids, Bases, and Salts. Key topics: pH scale; acid-base properties of water. Ka = acid ionization constant; Kb = base ionization constant. Polyprotic acids. BrOnsted Acids and Bases. Acid: proton donor. Base: proton acceptor acid/base reaction: proton transfer. Each side of the reaction has an acid and a base !
The chemistry of acids and bases is an area of fundamental importance in chemistry. In this experiment you will study acid-base equilibria by deter- mining the pH of a number of acids and bases and their mixtures and by per- forming a pH titration. In particular, the aims of this experiment are: 1. To demonstrate that only a
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