Graph Titrations

Strong Acid-Strong Base Titration (neutral solution)

A=initial pH of acid, pH=-log [H₃O⁺]

B= Base is added until acid is neutralized. Account for moles of base added moles of unnaturalized H₃O⁺ determine the pH.

C= equivalence point moles of acid = moles of base, pH=7

D= pH will be based on OH^- left in solution.

Weak Acid-Strong Base Titration (Acidic Solution)

A= pH depends on concentration of weak acid, using ICE table

B= HA+OH^- ←→A^-+H₂O. Buffer region, use H-H equation to calculate pH at ½ way point (1/2 way point pH=pK_a)

C= Equivalence point, pH will depend on [A^-] use ICE table K_b

D= pH determined by [OH^-]

Weak Base-Strong Acid Titration (Basic Solution)

A= pH depends on [weak base] use ICE table K_b

B= A^-+H₃O⁺<-> HA+ H₂O. Buffer region. use H-H equation to calculate pH at 1/2 way point [HA]=[A^-]. pH=pK_a

C= equivalence point pH will depend on [HA] use ICE table and K_a

D= All Base is neutralized. HA will remain and so will H₃O⁺. [H₃O⁺] will determine the pH of the solution.

Titration of a Weak Polyprotic Acid

Polyprotic acids have 2 buffer regions

The top pH is determined by [OH^-]

All three can exist at the same time