HI

HClO₄ (Perchloric)

 HBr

HCl

H₂SO₄ (Sulfuric)

HClO₃ (Chloric)

HNO₃ (Nitric)

• A substance that reacts essentially, completely with water to produce H₃O⁺.
• The proton donating power of HA is greater than that of H₃O⁺.

• A substance that is only partially deprotnated in water.
• The proton donating ability of HA is weaker than that of H₃O⁺

• A substance that reacts essentially completely with water to produce OH^- - it is completely protonated in water.

• The proton accepting power of A^- is greater than that of OH^-.

• Acid - Any species capable of donating an electron pair.
• Base - Any species capable of donating a pair of electrons.

• Acid - A proton donator.
• Base - A proton acceptor.

• Can be viewed as a special case of Lewis definiton

• Acid - A compund that produces H₃O⁺ (hydronium) when dissolved in water.
• Base - A compound that produces OH^- (hydroxide) in aqueous solution.

• A substance that is only partially deprotonated in water.
• The proton accepting power of A^- is less than that of OH^-.

• H₃O⁺ is the strongest acid that can exist in water and OH^- is the strongest base that can exist in water.
• An acid/base is strong if it is stronger than the conjugate acid/base of the solvent.

• A buffer solution is any solution that maintains an approximately constant pH despite small additions of acid/base or dilution
• Typically, a buffer contains a weak acid and conjugate weak base in approximately equal concentrations

• pH = pK_a - log₁₀([HA]_o/[A^-]_o)
• pOH = pK_b - log₁₀([A^-]_o/[HA]_o)
• HA and A^- represent conjugate acids and bases
• Equation may be applied towards buffers and the early stages of titrations

• Typically, a weak acid that has sharply different colors in its associated and dissociated states.
• When pH (of entire soln) = K_in, the concentrations of both states will be equal (both colors)
• When pH>K_in, [In^-]>[HIn]
• When pH<K_in, [In^-]<[HIn]

• Point in a titration when the acid/base has been completely neutralized by the base/acid.
• C_AV_A=C_BV_B

• The point in a titration at which exactly half the acid/base has been neutralized by the base/acid.
• pH = pK_a
• pOH = pK_b

• The pH of an amphiprotic salt solution is equal to the average of the pK_a's of the salt and its conjugate acid.
• pH = 1/2(pK_a1+pK_a2)