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Bronsted Lowry Acid and Base quiz

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  • What is the main idea behind the Bronsted-Lowry definition of acids?
    Bronsted-Lowry defines acids as proton (H+) donors. This means acids give away an H+ ion.
  • How does the Bronsted-Lowry definition of bases differ from the Arrhenius definition?
    Bronsted-Lowry defines bases as proton (H+) acceptors, not requiring OH-. Arrhenius defines bases as substances that produce OH- in water.
  • What is a proton in the context of Bronsted-Lowry theory?
    A proton refers to an H+ ion. It is the particle donated or accepted in acid-base reactions.
  • Can Bronsted-Lowry acids and bases exist in non-aqueous solutions?
    Yes, Bronsted-Lowry theory applies to solutions beyond just water. Arrhenius theory is limited to aqueous solutions.
  • What is a conjugate acid-base pair?
    A conjugate acid-base pair consists of two species that differ by only one hydrogen ion (H+). One is the acid, and the other is its conjugate base.
  • How do H2O and OH- form a conjugate acid-base pair?
    H2O and OH- differ by one H+ ion. H2O is the acid, and OH- is its conjugate base.
  • What is the relationship between H3O+ and H2O in Bronsted-Lowry theory?
    H3O+ and H2O are a conjugate acid-base pair. H3O+ is the acid, and H2O is its conjugate base.
  • Why does a base accept H+ according to Bronsted-Lowry?
    A base accepts H+ because it has lone pairs or a negative charge. These features attract the positive H+ ion.
  • Do Arrhenius acids and Bronsted-Lowry acids always agree?
    Yes, Arrhenius acids are also Bronsted-Lowry acids. Both definitions agree that acids donate or increase H+.
  • What is the key disagreement between Arrhenius and Bronsted-Lowry regarding bases?
    Arrhenius requires bases to produce OH- in water, while Bronsted-Lowry only requires bases to accept H+.
  • What is required for a substance to be a Bronsted-Lowry base?
    It must be able to accept a proton (H+). This usually means it has lone pairs or a negative charge.
  • What does it mean for conjugate acid-base pairs to differ by one hydrogen?
    It means one member of the pair has one more H+ than the other. The acid has the extra H+, the base has one less.
  • Why are Bronsted-Lowry acids and bases considered more general than Arrhenius acids and bases?
    Bronsted-Lowry theory applies to all solutions, not just water. Arrhenius is limited to aqueous solutions.
  • What is the significance of lone pairs in Bronsted-Lowry bases?
    Lone pairs allow bases to accept H+ ions. This is essential for their role as proton acceptors.
  • How did Bronsted-Lowry improve the definition of acids and bases?
    They expanded the definition to include proton donors and acceptors, not just substances that produce H+ or OH- in water. This made the theory applicable to more types of reactions.