The nature of acid and bases

• Arrhenius acid/base theory: acids produce hydrogen ions in aqueous solution, and bases produce hydroxide ions — limited application
• Brønsted-Lowry acid/base theory: acids are proton (H+) donors, and bases are proton acceptors
• Lewis acid/base theory: acids are electron-pair acceptors and bases are electronpair donors
• Conjugate acid is the base that is protonated
• Conjugate acid is the base that is protonated
• Conjugate acid-base pair: Two substance related to each other by accepting and donating a single proton
• Strong acid: equilibrium lies far to the right, yields a weak conjugate base
• Weak acid: equilibrium lies far to the left; the weaker the acid, the stronger its conjugate base
• he conjugate acid adds one proton

  The conjugate base substracts one proton
• The higher the Kb, the stronger the substance is as a base
• The higher the Ka, the stronger the acid is, and the weaker its conjugate base is.
• Equilibrium lies far to the right, The acid is stronger
• Equilibrium lies far to the left, The base yields a stronger reaction