Chemistry: Arrhenius, Bronsted-Lowry, and Lewis Acids and Bases

Consider the reaction below. HI + H2O mc014-1.jpg H3O+ + I- Which is an acid-conjugate base pair? HI and H2O H2O and H3O+ H3O+ and I- HI and I-

D : HI and I-

Which statement describes the Arrhenius interpretation of acids and bases?

D : It is limited to situations that involve aqueous solutions or specific compounds.

Which of the following would most likely act as a Bronsted-Lowry acid?

*Not D*

Which reaction displays an example of an Arrhenius base?

A : NaOH(s) mc005-1.jpg Na+(aq) + OH-(aq)

What is the Bronsted-Lowry definition of an acid?

A : a compound that donates protons

Which term describes a substance that increases the concentration of hydroxide ions in solution?

B : Arrhenius definition of a base

Which statement best describes a Bronsted-Lowry base?

B : It must accept protons to form a conjugate acid.

Consider the reaction below. HClO3 + NH3 mc012-1.jpg NH4+ + ClO3- Which is a base-conjugate acid pair? NH3 and ClO3- NH3 and NH4+ HClO3 and NH3 HClO3 and NH4+

B : NH3 and NH4+

A chemist lectures about the following definition for acids and bases. The acid-base behavior is analyzed in terms of how electrons are transferred between compounds rather than in terms of how hydrogen ions are transferred. What is the chemist defining?

C : the Lewis concept of acids and bases