Buffer Solution and pH Calculation
What is the pH of the buffer after 0.750 mol of H⁺ have been added?
Final answer:
The addition of H⁺ ions will not significantly change the pH of the buffer solution due to the buffer's ability to resist changes in pH. A quantitative answer would require calculations using the Henderson-Hasselbalch equation.
Answer:
After adding 0.750 mol of H⁺ ions to the buffer solution, the pH will remain relatively constant. This is because the buffer system is composed of a weak acid (HC₇H₅O₂) and its conjugate base (NaC₇H₅O₂), which can neutralize the additional H⁺ ions without a significant change in pH.
A buffer solution is a solution that can resist changes in pH when a small amount of acid or base is added. It consists of a weak acid and its conjugate base, which react with H⁺ or OH⁻ ions to maintain the pH within a certain range.
In this case, the addition of 0.750 mol of H⁺ ions to the buffer will be neutralized by the base present in the solution, preventing a significant change in pH. The buffer's capacity to maintain pH stability is due to the equilibrium between the weak acid and its conjugate base.
To calculate the exact pH after adding 0.750 mol of H⁺ ions, you would need to use the Henderson-Hasselbalch equation, taking into account the initial concentrations of the acid and the base. This equation allows you to determine the pH of a buffer solution based on the concentrations of the acidic and basic components.
Overall, the buffer system effectively resists changes in pH by neutralizing added H⁺ or OH⁻ ions, making it essential in various chemical and biological processes where pH stability is crucial.