Question

In each row, check the box under the compound that can reasonably be expected to be more acidic in aqueous solution, e.g. have the larger Ka

a) HCH3CO2 vs HCH3SO2

b) H3PO4 vs H3PO3

c HClO2 vs HClO

Answer 1

More acidic compounds typically have structures that stabilize the negative charge left behind after deprotonation. Factors influencing acid strength include the electronegativity of the atoms involved and the presence of additional oxygen atoms.

Step-by-step explanation:

The subject in question relates to the concept of acid strength and acid dissociation constants (Ka) in aqueous solutions, fundamental topics in Chemistry. Specifically, it requires predicting which compound in each pair would be more acidic based on structural considerations and known principles such as periodic trends and the presence of electronegative elements that can stabilize the anion left behind after proton donation.

• HCH3CO2 (acetic acid) vs HCH3SO2 (methanesulfonic acid): Methanesulfonic acid is more acidic because sulfur is more electronegative than carbon, stabilizing the negative charge on its conjugate base.
• H3PO4 (phosphoric acid) vs H3PO3 (phosphorous acid): Phosphoric acid is more acidic due to the presence of an additional oxygen, which can stabilize the negative charge after deprotonation.
• HClO2 (chlorous acid) vs HClO (hypochlorous acid): Chlorous acid is more acidic because it has more oxygen atoms, enhancing the stability of the conjugate base through greater electron delocalization.