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Bronsted Lowry Acid and Base quiz #1

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Terms in this set (29)

  • Bronsted and Lowry defined acids and bases in terms of what?
    Bronsted and Lowry defined acids and bases in terms of proton (H+) transfer: acids are proton donors and bases are proton acceptors.
  • Whose definition of acids and bases emphasizes the role of protons?
    The Bronsted-Lowry definition emphasizes the role of protons (H+) in defining acids and bases.
  • Which sentence is true of all Bronsted-Lowry bases?
    All Bronsted-Lowry bases are proton (H+) acceptors.
  • Which species can act as a Bronsted-Lowry base?
    Any species that can accept a proton (H+), such as those with lone pairs or a negative charge, can act as a Bronsted-Lowry base.
  • What must be present in a Bronsted-Lowry base?
    A Bronsted-Lowry base must have the ability to accept a proton (H+), typically through lone pairs or a negative charge.
  • What is true about a Bronsted-Lowry base?
    A Bronsted-Lowry base accepts a proton (H+) from an acid.
  • How are acids described according to the Bronsted-Lowry definition?
    According to the Bronsted-Lowry definition, acids are described as proton (H+) donors.
  • Which of the choices describes a Bronsted-Lowry base?
    A Bronsted-Lowry base is a substance that accepts a proton (H+).
  • Which statement best describes a Bronsted-Lowry base?
    A Bronsted-Lowry base is a proton (H+) acceptor.
  • What is the Bronsted-Lowry definition of an acid?
    A Bronsted-Lowry acid is a substance that donates a proton (H+).
  • What is the Bronsted-Lowry definition of a base?
    A Bronsted-Lowry base is a substance that accepts a proton (H+).
  • What is the conjugate base of HCO3−?
    The conjugate base of HCO3− is CO3^2−, formed by the loss of one H+ ion.
  • What is the conjugate acid of ClO−?
    The conjugate acid of ClO− is HClO, formed by the addition of one H+ ion.
  • What is the conjugate acid of HSO4−?
    The conjugate acid of HSO4− is H2SO4, formed by the addition of one H+ ion.
  • What is the conjugate base of H2CO3?
    The conjugate base of H2CO3 is HCO3−, formed by the loss of one H+ ion.
  • What is the conjugate base of HI?
    The conjugate base of HI is I−, formed by the loss of one H+ ion.
  • What is the conjugate acid of NH3?
    The conjugate acid of NH3 is NH4+, formed by the addition of one H+ ion.
  • What is the conjugate base of HI?
    The conjugate base of HI is I−, formed by the loss of one H+ ion.
  • What is the conjugate base of HF?
    The conjugate base of HF is F−, formed by the loss of one H+ ion.
  • What is the conjugate base of OH−?
    The conjugate base of OH− is O^2−, formed by the loss of one H+ ion.
  • What is the conjugate acid of HSO3−?
    The conjugate acid of HSO3− is H2SO3, formed by the addition of one H+ ion.
  • What is the conjugate base of NH4+?
    The conjugate base of NH4+ is NH3, formed by the loss of one H+ ion.
  • What is the conjugate acid of C6H5NH2?
    The conjugate acid of C6H5NH2 is C6H5NH3+, formed by the addition of one H+ ion.
  • What is the Bronsted-Lowry definition of a base?
    A Bronsted-Lowry base is a proton (H+) acceptor.
  • What is a Bronsted-Lowry acid?
    A Bronsted-Lowry acid is a proton (H+) donor.
  • What is the Bronsted-Lowry definition of an acid?
    A Bronsted-Lowry acid is a substance that donates a proton (H+).
  • What is a conjugate acid-base pair?
    A conjugate acid-base pair consists of two species that differ by only one hydrogen ion (H+).
  • What is the conjugate acid of HPO2^2−?
    The conjugate acid of HPO2^2− is H2PO2−, formed by the addition of one H+ ion.
  • How do Bronsted-Lowry acids and bases differ from Arrhenius acids and bases?
    Bronsted-Lowry acids are proton donors and bases are proton acceptors, while Arrhenius acids increase H+ concentration in water and bases increase OH− concentration. Bronsted-Lowry definitions apply beyond aqueous solutions.