Chemistry Buffers Quiz

Buffers

• Buffers are solutions resisting pH changes when acids or bases are added.
• Typically, a buffer solution consists of a weak acid and a salt of that acid or a weak base and a salt of that base.
• Buffer action is the solution's ability to resist pH changes.

Buffer Action Examples

• A sodium chloride solution is not a buffer because adding acid or base significantly alters pH.
• A weak acid (acetic acid) mixed with its salt (sodium acetate) forms a buffer. If a strong acid is added, the H+ ions are neutralized by the acetate ions, changing pH minimally.
• A weak base (ammonium hydroxide) mixed with its salt (ammonium chloride) forms a buffer. If a strong acid is added, the H+ ions are neutralized by the base, with minimal pH change. If a strong base is added, OH- ions are neutralized by the ammonium ions.

The Buffer Equation

• The pH of a buffer solution and the pH change due to adding acid or base can be calculated using a buffer equation.
• The equation considers the effect of a salt on the ionization of a weak acid or base if they share a common ion.
• For a weak acid and its salt: pH = pKa + log ([salt]/[acid])
• For a weak base and its salt: pH = pKw - pKb + log ([base]/[salt])

Buffer Capacity

• Buffer capacity (β) measures a buffer's resistance to pH change.
• A higher capacity means more acid/base is needed to change pH.
• The capacity is related to the amount of strong acid/base needed to shift pH by one unit in a liter of buffer solution.
• Van Slyke's equation calculates buffer capacity: β = 2.303C (Ka[H3O+]) / (Ka + [H3O+])²

Maximum Buffer Capacity

• Maximum buffer capacity (βmax) occurs when pH equals the pKa.
• βmax = 0.576C, where C is the total buffer concentration.

Buffer Capacity Factors

• Buffer capacity depends on the ratio of salt to acid/base, and total buffer concentration.
• Optimal buffer ratio is 1:1 (salt:acid or base).
• Higher total concentration results in greater buffer capacity (more acid/base needed to change pH).

Buffers in Biological Systems

• Blood pH is maintained around 7.4 by primary and secondary buffers.
• Plasma contains carbonic acid/bicarbonate and protein buffers.
• Erythrocytes contain hemoglobin/oxyhemoglobin and phosphate buffers.
• Experimentally, whole blood has a buffer capacity of about 0.039 gram equivalents per liter/pH unit, with most from cells.
• pH outside of 7.0-7.8 is a danger sign.

Pharmaceutical Buffers

• Sorensen proposed using sodium phosphate salts to create pH 6-8 buffers, made isotonic using sodium chloride.
• Hind-Goyan used boric acid, sodium borate, and sodium chloride for pH 7-9 ophthalmic solutions.

Preparation of Pharmaceutical Buffers

• Choose an optimal pH.
• Select a weak acid or base with a pKa near the desired pH and is nontoxic, physically/chemically compatible with other additives.
• Calculate the salt/acid/base ratio using the buffer equation.
• Determine the total buffer concentration needed for the desired capacity using Van Slyke's equation. (0.05M is often enough; 0.01-0.1 sufficient)

Buffer Capacity Impact on Tissue Irritation

• Solutions for tissues/parenteral use are prone to irritation if their pH or buffer capacity is incompatible with the relevant body fluid's pH or capacity.
• Lower buffer capacity, less volume in contact with the body fluid, or larger buffer capacity of the contacted body fluid all contribute to reduced irritation risk.

Drug Stability

• Aqueous drug instability can arise from the catalytic effect of acids or bases.
• Cocaine decomposition minimizes around pH 2-5.
• Thiamine HCl is unstable above a pH of 5.

Drug Activity

• Drugs like mandelic acid, benzoic acid, and salicylic acid are more effective as antibacterial agents in their unionized form at acidic pH.

Drug Absorption

• Ionization degree and lipoid solubility affect rate of drug absorption through cellular membranes.
• Weak organic acids/bases readily dissolve in lipids and pass through lipid-like cellular membranes in their non-ionized form.

pH and Solubility

• Ionization of weak acids/bases depends on their pKa and solution pH.
• Ionization degree influences many pharmaceutical drug properties.
• At acidic (low) pH, bases exist mostly in ionic form, tending to increase solubility in aqueous solutions.

Test your knowledge about buffers and their role in maintaining pH levels in solutions. This quiz covers the types of buffer solutions, examples, and the buffer equation. Challenge yourself and see how well you understand this important concept in chemistry!