Given the following Bronsted-Lowery acid-base reaction and its corresponding equilibrium constant, which substance is the strongest acid ?
CH ₃CH ₂ NH₃+ + ClO₂₁ - CH ₃CH ₂ NH₂ + HClO ₂ K = 2.1 10 - 9

Question

Given the following Bronsted-Lowery acid-base reaction and its corresponding equilibrium constant, which substance is the strongest acid ?
CH ₃CH ₂ NH₃+ + ClO₂₁ -

CH ₃CH ₂ NH₂ + HClO ₂ K = 2.1 10 - 9

Quizplus · Accepted Answer

The strength of an acid is determined by its ability to donate a proton (H+). In this reaction, the acid is the compound that donates a proton, while the base is the compound that accepts a proton. The dissociation of HClO2 produces H+ and ClO2-, making it the stronger acid compared to CH3CH2NH3+, which only becomes CH3CH2NH2 after donating a proton. The equilibrium constant (K) value does not affect the strength of the acid, as it only measures the extent of the reaction at equilibrium. Therefore, the answer is D) HClO2.

Given the Following Bronsted-Lowery Acid-Base Reaction and Its Corresponding Equilibrium