Ask Question
30 April, 01:19

What makes the Arrhenius acid and an Arrhenius base definition incomplete or lacking

+3
Answers (1)
  1. 30 April, 02:49
    0
    See Explanation

    Explanation:

    The Arrhenius acid-base theory defines an acid as a compound which when added into water increases the hydronium ion (H₃O⁺) concentration and the base as a compound which when added into water increases the hydroxide (OH⁻) ion concentration. As such, an acid-base reaction is limited to proton transfer to only OH⁻ ions forming water. Such would imply that all acid-base reactions produce water only in addition to a salt. This is not always the case as conjugate base anions for many substances can receive proton transfer.

    Example: The reaction HOAc + NaCN = > HCN + OAc - will occur in aqueous media because the proton (H⁺) on acetic acid (HOAc) will transfer to the cyanate ion forming hydrocyanic acid (HCN). Such occurs because the CN⁻ ion is a stronger conjugate base than the acetate ion (OAc⁻) and forms the more stable weak acid. Such is the basis of the Bronsted-Lowry Acid-Base system and states that an acid (proton donor) will transfer its ionizable hydrogen to a conjugate base (proton acceptor) if the transfer forms a weaker acid.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “What makes the Arrhenius acid and an Arrhenius base definition incomplete or lacking ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers