Bronsted-Lowry Theory

• Bronsted Lowry Theory


  Alternate acid-base theory
• Acid


  Proton (H+) donor - Gives protons (DONATE)
• Base


  Proton (H+) acceptor - Takes protons (ACCEPT)
• Protons refers to Hydrogen ions
• When acid dissolves in water

  1. Water acts as Bronsted Lowry base & removes a Proton (H) from acid

  2. Result: conjugate base of the acid & hydion ion
• Conjugate Acids & Bases

  • Acid removes H+
  • Base adds H+
• Amphiprotic Substance


  Can act like an acid or a base (can behave as a proton donor/acceptor)
• Strong acids & bases


  • Completely dissociated in water to make a lot of H+ or OH-
• Weak acids & bases

  • Only dissociate partially in water to make a small amount of H+ or OH-
• Acid with higher molarity


  Will produce more ions than lower molarity acid in a solution
• Acid with higher molarity


  Is a stronger electrolyte with greater electrical conductivity
• Strength


  Amount of ions a substance makes when it breaks down
• Concentration


  Amount of substance initially, before it breaks down
• Strength and concentration are usually measured in molarity (M/L)
• B - Bases

  A - Accept

  A - Acids

  D - Donate
• Bronsted-Lowry Theory = Alternate Acid-Base Theory
• Gain/Accept H+ ---> Base
• Lose/give away H+ ---> Acid
• Acids: Proton donors
• Bases: proton acceptor (receiver)
• Depending on the direction the reaction is in, the one who's going to donate an H+ to the other substance is the acid & the one who's going to accept that H+ on the other side of equation is the base
• Conjugate acid-base pairs

  • When substances differ only by a H+
• BL Acids always have on more H+ than their conjugate base

  Its always; ACID/CONJUGATE BASE
• BL bases always have one less H+ than their conjugate acid.

  its always: BASE/ CONJUGATE ACID
• To find Acid ---> Add H+ to substance
• To find base ---> Remove H+ to substance