This preview shows page 1. Sign up to view the full content.
Unformatted text preview: 3 + <--> (R)-NH 2 + H + 1) At which pH would the charged form be predominant? ( no full credit without explanation ) pH < pKa. Once pH > pKa, the basic (deprotonated, neutral) form is predominant. or the acid form is charged, so the uncharged (basic form) is predominant pH > 8 2) At pH=7, how would you calculate the ratio of base to acid? (only equation is needed) pH = pKa + log([base]/[acid]) 3) Lets assume (R)-NH 3 + is a drug. Its absorption requires passage through a membrane. At which pH will the drug be optimally absorbed? Why? pH > 8 To go through a membrane, the drug needs to be deprotonated (neutral) because of the hydrophobic environment of the membrane. " G = " G ! + RT ln Q...
View Full Document
- Spring '07