What form of a drug is more lipid-soluble, and thus would remain trapped within a compartment where the pH does not favor the lipid-soluble form? a) Strong acid (A-) b) Weak acid (A-) c) Neutral (AH and B) d) Weak base (BH+) e) Strong base (BH+)
Added by Larry M.
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Drugs can exist in different forms depending on their pH and the pKa of the drug. Weak acids (HA) can dissociate into their anionic form (A-) in a basic environment, while weak bases (BH+) can become protonated in an acidic environment. Show more…
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Supreeta N.
Even though both $\mathrm{NH}_{3}$ and $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}$ are weak bases, NH_{3} is a much stronger acid than $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}$ . Which of the following is correct at equilibrium for a solution that is initially 0.10$M$ in $\mathrm{NH}_{3}$ M in $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} ?$ $$ \begin{array}{l}{\text { (a) }\left[\mathrm{OH}^{-}\right]=\left[\mathrm{NH}_{4}^{+}\right]} \\ {\text { (b) }\left[\mathrm{NH}_{4}^{+}\right]=\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\right]} \\ {\text { (c) }\left[\mathrm{OH}^{-}\right]=\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}+\right]} \\ {\text { (d) }\left[\mathrm{NH}_{3}\right]=\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\right]} \\ {\text { (e) both a and b are correct }}\end{array} $$
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