The liver is a metabolic machine and often inactivates drugs on their way from the gastrointestinal (GI) tract to the body. This is called the first-pass effect.
Orally administered drugs are absorbed from the gastrointestinal (GI) tract. The blood from the GI tract then travels through the liver, the great chemical plant in the body. Many drugs that undergo liver metabolism will be extensively metabolized during this passage from the GI tract to the body. This effect of liver metabolism is called the first-pass effect.
HOW DRUGS CROSS MEMBRANES
There are several useful routes of drug administration, but almost all require that the drug cross a biological membrane to reach its site of action.
Drugs cross membranes by passive diffusion or active transport.
This statement is somewhat simplified, but it provides a useful starting point. Passive diffusion requires a concentration gradient across the membrane. The vast majority of drugs gain access to their site of action by this method.
A drug tends to pass through membranes if it is uncharged.
Uncharged drugs are more lipid soluble than charged drugs. In addition, most drugs are weak acids or weak bases.
For a weak acid, when the pH is less than the pK, the protonated form (nonionized) predominates. When the pH is greater than the pK, the unprotonated (ionized) form predominates.
Weak acids are hydrogen ion donors; they are happy to give up a hydrogen ion and become charged. If you have trouble remembering whether they become charged or uncharged after donating their hydrogen ion, think of a strong acid, such as HCl. As you know, when you put HCl into water, it immediately turns into H+ and Cl−. Use this example to remember that weak acids donate a hydrogen ion and become charged.
Remember the pK? That is the equilibrium constant (of course, the p means we’ve taken the negative log of the equilibrium constant). When the pH is equal to the pK, there are equal amounts of weak acid in the ionized and nonionized forms. If we decrease the pH by adding more H+, we will drive the equilibrium for the weak acid more to the left, which is the nonionized (uncharged) form.
If we take away H+, making the pH higher, we will drive the equilibrium toward the right. This increases the concentration of the ionized form of the weak acid (Figure 3–1).
The relationship between the pH and the degree of ionization of a weak acid is presented. When the pH is higher than the pK for the acid, the charged form of the acid predominates.