CHEM2: Acid-Base Equilibria

• Acids - Have a sour taste.
• Vinegar and citric fruits are examples of acids.
• Bases - Have a bitter taste and feel slippery.
• Arrhenius acid - A substance that produces H+ or H3O+ in water.
• Arrhenius base - A substance that produces OH- in water.
• Bronsted acid - A proton (H+) donor.
• Bronsted base - A proton (H+) acceptor.
• Lewis acids - Electron pair acceptors.
• Lewis bases - Electron pair donors.
• Water is amphoteric.
• Amphiprotic - Can act as an acid or base. Can be a proton donor or acceptor.
• The equilibrium expression for the autoionization of water: Kc=[H3O+][OH-] or Kc=[H+][OH-]
• Kw - The ion-product constant.
• The value of the ion-product constant: Kw=1.0x10^-14
• Neutral - [H+]=[OH-]
• Acidic - [H+]>[OH-]
• Basic - [H+]<[OH-]
• Neutral - [H+]=[OH-] = 1.0x10^-7
• Acidic - [H+]>1.0x10^-7
• Basic - [H+]<1.0x10^-7
• Basic - [OH-]>1.0x10^-7
• Acidic - [OH-]<1.0x10^-7
• pH - Means power of hydrogen. A method of reporting hydrogen ion concentration.
• Formula of pH: pH=-log[H+]
• Neutral pH is 7.00.
• Acidic pH is below 7.00.
• Basic pH is above 7.00.
• Formula of pOH: pOH=-log[OH-]
• What is the sum? pH+pOH=14
• Indicator - A compound that has one color in its acid form and another color in its basic form.
• 6 Monoprotic Acids: HCl, HBr, HI, HNO3, HClO3, and HClO4
• 1 Diprotic Acid: H2SO4
• Monoprotic - One hydrogen.
• Diprotic - Two hydrogen.
• Strong acids are strong electrolytes.
• All strong acids ionize completely in solution (100% dissociation).
• Complete what's missing. [H+]=10^-pH
• Complete what's missing. [OH-]=10^-pOH
• Strong Bases - These substances dissociate completely in aqueous solution.
• Ka - The acid-dissociation constant.