Question

Consider a buffer solution where [weak acid] \(>\) [conjugate base]. How is the pH of the solution related to the \(\mathrm{p} K_{\mathrm{a}}\) value of the weak acid? If [conjugate base] \(>\) [weak acid], how is pH related to \(\mathrm{p} K_{\mathrm{a}} ?\)

Short answer

In a buffer solution, the relationship between pH and pKa can be described using the Henderson-Hasselbalch equation: \(pH = pKa + \log\frac{[\text{conjugate base}]}{[\text{weak acid}]}\). When [weak acid] > [conjugate base], the pH of the solution will be lower than the pKa of the weak acid. Conversely, when [conjugate base] > [weak acid], the pH of the solution will be higher than the pKa of the weak acid.

Step-by-step solution

Henderson-Hasselbalch equation

This equation is given as follows: \(pH = pKa + \log\frac{[\text{conjugate base}]}{[\text{weak acid}]}\) Now, let's analyze the given scenarios. Case 1: The concentration of the weak acid is greater than the concentration of the conjugate base.

Analyzing the relationship

In this case, since [weak acid] > [conjugate base], the fraction \(\frac{ [\text{conjugate base}]}{[\text{weak acid}]}\) will be less than 1. Consequently, the value of the logarithm will be negative because \(\log(x) < 0\) if \(0 < x < 1\). Therefore, in this scenario, the pH of the solution will be lower than the pKa of the weak acid. Case 2: The concentration of the conjugate base is greater than the concentration of the weak acid.

Analyzing the relationship

In this case, since [conjugate base] > [weak acid], the fraction \(\frac{ [\text{conjugate base}]}{[\text{weak acid}]}\) will be greater than 1. Consequently, the value of the logarithm will be positive because \(\log(x) > 0\) if \(x > 1\). Therefore, in this scenario, the pH of the solution will be higher than the pKa of the weak acid. In conclusion, when [weak acid] > [conjugate base], the pH of the solution will be lower than the pKa of the weak acid. And when [conjugate base] > [weak acid], the pH of the solution will be higher than the pKa of the weak acid.

Key concepts

Henderson-Hasselbalch equation

The Henderson-Hasselbalch equation is a vital tool in chemistry for understanding how pH relates to concentrations of acid and base in a solution. This equation is expressed as:\[ pH = pKa + \log\frac{[\text{conjugate base}]}{[\text{weak acid}]} \]In practice, this formula helps determine the pH of a buffer solution. A buffer solution is one that can resist changes in its pH when small amounts of acid or base are added. The equation uses the logarithmic ratio of the concentrations of the conjugate base and the weak acid. This mathematical relationship shows that the pH increases as the concentration of the conjugate base goes up compared to the weak acid, and decreases if the weak acid concentration is greater. Understanding this balance is essential for creating solutions that maintain a stable pH, which is crucial for various chemical reactions and processes.

pH and pKa relationship

The relationship between pH and pKa is fundamental in understanding acid-base chemistry. The \( \text{pKa} \) is a measure of the strength of an acid — the lower the \( \text{pKa} \), the stronger the acid. When you look at the equation \[ \text{pH} = \text{pKa} + \log\frac{[\text{conjugate base}]}{[\text{weak acid}]} \]it becomes clear that the \( \text{pKa} \) value serves as a central point or reference.

- If the concentrations of the conjugate base and weak acid are equal, \( \log\left(1\right) = 0 \), meaning the pH of the solution equals the \( \text{pKa} \). - If \([\text{conjugate base}] > [\text{weak acid}], \log\) is positive, making the pH higher than the \( \text{pKa} \).- Conversely, if \([\text{weak acid}] > [\text{conjugate base}], \log\) is negative, resulting in a pH lower than the \( \text{pKa} \).
The relationship between pH and \( \text{pKa} \) is crucial because it allows scientists to predict how changes in concentration will affect pH, which is important in both lab and industrial settings.

Weak acid and conjugate base concentration

The concentrations of weak acids and their conjugate bases are integral in determining the pH of a buffer solution. A weak acid only partially dissociates in water, establishing an equilibrium between the acid \( (HA) \) and its conjugate base \( (A^-) \). This dynamic equilibrium is described by the equation:\[ HA \iff H^+ + A^- \]In a buffer solution, the concentration of the weak acid and its conjugate base can be adjusted to maintain a desired pH level. - **Higher Weak Acid Concentration:** When the concentration of the weak acid is greater than its conjugate base, the pH will be lower than the \( \text{pKa} \), showing a net increase in acidity.- **Higher Conjugate Base Concentration:** If the concentration of the conjugate base surpasses the weak acid, the pH will rise above the \( \text{pKa} \), indicating a more basic solution.The ability to control pH by altering these concentrations is why buffer solutions are incredibly useful in areas like biochemistry, pharmaceuticals, and environmental science, where exact pH conditions can be critical.