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Solutions for Chapter 18: Acid-Base Equilibria

Chemistry: The Molecular Nature of Matter and Change | 5th Edition | ISBN: 9780073048598 | Authors: Martin S. Silberberg

Full solutions for Chemistry: The Molecular Nature of Matter and Change | 5th Edition

ISBN: 9780073048598

Chemistry: The Molecular Nature of Matter and Change | 5th Edition | ISBN: 9780073048598 | Authors: Martin S. Silberberg

Solutions for Chapter 18: Acid-Base Equilibria

Solutions for Chapter 18
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Textbook: Chemistry: The Molecular Nature of Matter and Change
Edition: 5
Author: Martin S. Silberberg
ISBN: 9780073048598

This expansive textbook survival guide covers the following chapters and their solutions. Chapter 18: Acid-Base Equilibria includes 189 full step-by-step solutions. Chemistry: The Molecular Nature of Matter and Change was written by and is associated to the ISBN: 9780073048598. This textbook survival guide was created for the textbook: Chemistry: The Molecular Nature of Matter and Change , edition: 5. Since 189 problems in chapter 18: Acid-Base Equilibria have been answered, more than 29577 students have viewed full step-by-step solutions from this chapter.

Key Chemistry Terms and definitions covered in this textbook
  • Antiaromatic compound

    A monocyclic compound that is planar or nearly so, has one 2p orbital on each atom of the ring, and has 4n p electrons in the cyclic arrangement of overlapping 2p orbitals, where n is an integer. Antiaromatic compounds are especially unstable

  • beta particles.

    See beta rays.

  • chemical changes

    Processes in which one or more substances are converted into other substances; also called chemical reactions. (Section 1.3)

  • complete ionic equation

    A chemical equation in which dissolved strong electrolytes (such as dissolved ionic compounds) are written as separate ions. (Section 4.2)

  • condensation reaction.

    A reaction in which two smaller molecules combine to form a larger molecule. Water is invariably one of the products of such a reaction. (24.4)

  • effusion

    The escape of a gas through an orifice or hole. (Section 10.8)

  • Energy

    The ability to do work.

  • ferromagnetism

    A form of magnetism in which unpaired electron spins align parallel to one another. (Section 23.1)

  • halogenation

    A reaction that involves the addition of X2 (either Br2 or Cl2) across an alkene.

  • Hammond postulate

    In an exothermic process the transition state is closer in energy to the reactants than to the products, and therefore the structure of the transition state more closely resembles the reactants. In contrast, the transition state in an endothermic process is closer in energy to the products, and therefore the transition state more closely resembles the products.

  • Henderson-Hasselbalch equation

    An equation that is often employed to calculate the pH of buffered solutions: pH = pKa + log 3conjugated base4 3acid4

  • ideal-gas equation

    An equation of state for gases that embodies Boyle’s law, Charles’s law, and Avogadro’s hypothesis in the form PV = nRT. (Section 10.4)

  • isoprene

    2-Methyl-1,3-butadiene.

  • main-group elements

    Elements in the s and p blocks of the periodic table. (Section 6.9)

  • metallic hydrides

    Compounds formed when hydrogen reacts with transition metals; these compounds contain the hydride ion, H-. (Section 22.2)

  • net ionic equation

    A chemical equation for a solution reaction in which soluble strong electrolytes are written as ions and spectator ions are omitted. (Section 4.2)

  • ortho

    On an aromatic ring, the C2 position.

  • porphyrin

    A complex derived from the porphine molecule. (Section 23.3)

  • Stereoisomers

    Isomers that have the same molecular formula and the same connectivity of their atoms but a different orientation of their atoms in space

  • trivalent

    An element, such as nitrogen, that forms three bonds.

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