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Bronsted Lowry Acid and Base quiz

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Termini in questo insieme (15)

  • Who developed the Bronsted-Lowry definition of acids and bases, and in what year?
    Bronsted and Lowry developed their definition in 1923.
  • According to Bronsted-Lowry, what is an acid?
    A Bronsted-Lowry acid is a proton (H+) donor.
  • What does the term 'proton' refer to in Bronsted-Lowry theory?
    In Bronsted-Lowry theory, 'proton' refers to H+.
  • How does the Bronsted-Lowry definition of acid relate to the Arrhenius definition?
    Both definitions agree that acids have H+ and increase H+ concentration in solution.
  • What is the Bronsted-Lowry definition of a base?
    A Bronsted-Lowry base is a proton (H+) acceptor.
  • How does the Bronsted-Lowry definition of a base differ from the Arrhenius definition?
    Bronsted-Lowry bases accept H+, while Arrhenius bases must produce OH-.
  • Why can Bronsted-Lowry bases accept H+?
    They can accept H+ because they have lone pairs or a negative charge.
  • What is a conjugate acid-base pair?
    A conjugate acid-base pair consists of two species that differ by only one hydrogen atom.
  • Give an example of a conjugate acid-base pair involving water.
    H2O and OH- are a conjugate acid-base pair, differing by one H+.
  • How do H3O+ and H2O relate as conjugate acid-base pairs?
    H3O+ and H2O are conjugate acid-base pairs, differing by one H+.
  • Can Bronsted-Lowry acids and bases exist in non-aqueous solutions?
    Yes, Bronsted-Lowry acids and bases can exist in solutions not made up of water.
  • What is the main requirement for a Bronsted-Lowry acid?
    It must be able to donate an H+ (proton).
  • What is the main requirement for a Bronsted-Lowry base?
    It must be able to accept an H+ (proton).
  • How do Arrhenius acids compare to Bronsted-Lowry acids?
    All Arrhenius acids are also Bronsted-Lowry acids.
  • What is the key difference between conjugate acid-base pairs?
    They differ by only one hydrogen atom (H+).