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Solutions for Chapter Chapter 44: Sample Preparation

Quantitative Chemical Analysis | 8th Edition | ISBN: 9781429218153 | Authors: Daniel C. Harris

Full solutions for Quantitative Chemical Analysis | 8th Edition

ISBN: 9781429218153

Quantitative Chemical Analysis | 8th Edition | ISBN: 9781429218153 | Authors: Daniel C. Harris

Solutions for Chapter Chapter 44: Sample Preparation

Solutions for Chapter Chapter 44
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Since 1 problems in chapter Chapter 44: Sample Preparation have been answered, more than 20745 students have viewed full step-by-step solutions from this chapter. Chapter Chapter 44: Sample Preparation includes 1 full step-by-step solutions. This expansive textbook survival guide covers the following chapters and their solutions. This textbook survival guide was created for the textbook: Quantitative Chemical Analysis, edition: 8. Quantitative Chemical Analysis was written by and is associated to the ISBN: 9781429218153.

Key Chemistry Terms and definitions covered in this textbook
  • acidic oxide (acidic anhydride)

    An oxide that either reacts with a base to form a salt or with water to form an acid. (Section 22.5)

  • aldonic acid

    The product obtained when the aldehyde group of an aldose is oxidized.

  • beta particles.

    See beta rays.

  • broadband decoupling

    In 13C NMR spectroscopy, a technique in which all 13C!1H splitting is suppressed with the use of two rf transmitters.

  • catalyst.

    A substance that increases the rate of a chemical reaction without itself being consumed. (13.6)

  • chemical bond

    A strong attractive force that exists between atoms in a molecule. (Section 8.1)

  • chemical reactions

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

  • conjugate acid-base pair.

    An acid and its conjugate base or a base and its conjugate acid. (15.1)

  • coordination-sphere isomers

    Structural isomers of coordination compounds in which the ligands within the coordination sphere differ. (Section 23.4)

  • Dalton’s law of partial pressures

    A law stating that the total pressure of a mixture of gases is the sum of the pressures that each gas would exert if it were present alone. (Section 10.6)

  • energy-level diagram

    A diagram that shows the energies of molecular orbitals relative to the atomic orbitals from which they are derived. Also called a molecular-orbital diagram. (Section 9.7)

  • gauche conformation

    A conformation that exhibits a gauche interaction.

  • Gibbs free energy

    A thermodynamic state function that combines enthalpy and entropy, in the form G = H - TS. For a change occurring at constant temperature and pressure, the change in free energy is ?G = ?H - T?S. (Section 19.5)

  • hydride ion

    An ion formed by the addition of an electron to a hydrogen atom: H-. (Section 7.7)

  • Markovnikov addition

    In additionreactions, the observation that the hydrogen atomis generally placed at the vinylic position alreadybearing the larger number of hydrogen atoms.

  • Michael donor

    The nucleophile in a Michael reaction.

  • nucleophilic attack

    One of the four arrow-pushing patterns for ionic reactions.

  • Pauli exclusion principle

    No more than two electrons may be present in an orbital. If two electrons are present, their spins must be paired

  • Polypeptide

    A macromolecule containing many amino acid units, each joined to the next by a peptide bond

  • symmetry forbidden

    A reaction that disobeys conservation of orbital symmetry.

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