2.8
Zuur-base-evenwicht: op activiteit gebaseerde definitie van pH
Voor een ideale oplossing wordt de pH gedefinieerd als de negatieve logaritme van de waterstofionenconcentratie. Voor een niet-ideale oplossing moet b…
The definition of the pH of a solution as the negative logarithm of the hydrogen ion concentration is valid only for an ideal solution.
In practice, the pH measurement considers the negative logarithm of the hydrogen ion activity rather than concentration.
So, the pH can be more accurately redefined as the negative logarithm of the product of the hydrogen ion concentration and its activity coefficient.
In the case of pure water at 25 degrees C, the extremely low ionic strength suggests that the activity coefficients of the ions are close to one.
However, adding a salt like potassium chloride to the water increases the ionic strength of the solution, thus decreasing the activity coefficients.
It follows here that the hydrogen ion activity is slightly increased, corresponding to a decrease in the pH of the solution.
Notably, the addition of potassium chloride causes a negligible change in pH but a significant increase in the hydrogen ion concentration.
View the full transcript and gain access to JoVE Core videos
Q1: Why is the traditional pH definition based on hydrogen ion concentration considered incomplete?
The negative logarithm of hydrogen ion concentration applies only to ideal solutions. In real solutions, pH must account for hydrogen ion activity, which reflects the effective concentration of hydrogen ions. Activity incorporates both concentration and an activity coefficient, providing a more accurate representation of how hydrogen ions behave in solution.
Q2: How does adding salt to pure water affect pH and hydrogen ion concentration?
Adding salt like potassium chloride increases ionic strength, which decreases activity coefficients and increases hydrogen ion activity. This causes a slight pH decrease. However, the hydrogen ion concentration increases significantly, demonstrating that activity and concentration respond differently to ionic strength changes.
Q3: What is the relationship between activity coefficient and ionic strength in solutions?
Activity coefficients decrease as ionic strength increases. In pure water with extremely low ionic strength, activity coefficients approach one, making activity nearly equal to concentration. As ionic strength rises through electrolyte addition, activity coefficients drop further, reducing the activity coefficient's value and affecting the solution's effective hydrogen ion concentration.
Q4: How can pH be mathematically expressed using activity and concentration?
pH is defined as the negative logarithm of hydrogen ion activity. This can be expressed as the negative logarithm of the product of hydrogen ion concentration and its activity coefficient. This formulation accounts for non-ideal behavior and provides accurate pH measurements in real solutions where activity differs from concentration.
Q5: Why do activity coefficients remain close to one in pure water?
Pure water has extremely low ionic strength because few ions are present to interact with hydrogen ions. When ionic strength is very low, activity coefficients approach one, meaning hydrogen ion activity nearly equals its concentration. This approximation breaks down when electrolytes are added, increasing ionic strength and decreasing activity coefficients.
Q6: What distinguishes ideal solutions from non-ideal solutions in pH measurement?
Ideal solutions assume activity equals concentration, so pH depends solely on hydrogen ion concentration. Non-ideal solutions require considering hydrogen ion activity, which accounts for ion interactions through the activity coefficient. Real solutions behave non-ideally, especially at higher ionic strengths, making activity-based pH definitions more accurate.
Q7: Why does potassium chloride cause negligible pH change despite increasing hydrogen ion concentration?
Potassium chloride increases ionic strength, which decreases activity coefficients and increases hydrogen ion activity. Although hydrogen ion concentration rises significantly, the activity increase is slight because the activity coefficient decrease partially offsets the concentration increase. This demonstrates that pH depends on activity, not concentration alone.