Which of the following is a Brønsted-Lowry base, but not an Arrhenius base? (LO 16.1) (a) HNO3 (b) CsOH (c) CH3NH2 (d) CH3OH

The Brønsted-Lowry theory defines acids as proton (H+) donors and bases as proton acceptors. This theory broadens the definition of bases beyond those that simply produce hydroxide ions in solution, allowing for a wider range of substances to be classified as bases based on their ability to accept protons.

The Arrhenius theory classifies acids as substances that increase the concentration of hydrogen ions (H+) in aqueous solution and bases as substances that increase the concentration of hydroxide ions (OH-). This definition is more restrictive, as it only considers substances that dissociate in water to produce these ions, limiting the classification of bases.

To determine which substance is a Brønsted-Lowry base but not an Arrhenius base, one must analyze the ability of each option to accept protons without necessarily producing hydroxide ions in solution. This involves understanding the chemical structure and behavior of the compounds listed, particularly focusing on their ability to act as proton acceptors.