Describe how a buffer behaves. Your description should include an explanation of why the addition of NaOH to the HAc solution formed a buffer. What happens to the pH when a small quantity of a strong acid or base is added to a buffer solution? What happens to the pH of the buffer solution when a large quantity of acid or base is added? Explain your observations.
my answer so far is: Buffers are commonly at a neutral pH of 7. When it is added to a more acidic solution it will make the solution turn more basic, and vice versa. However, the buffer keeps the solution at a natural pH because it never stops the reaction from shifting; therefore, it is constantly going between basic and acidic to counteract each other.
Buffers are commonly at a neutral pH of 7; this is wrong. Buffers are usually equal to the pKa or pKb of the acid and its conjugate base, or the base and its conjugate acid. You are right: they do counter act the addition of an acid by by making more of its conjugate base, or the addition of base by making more of its conjugate acid to resist a change in pH. Google more information concerning this.
Buffers are solutions that are able to resist changes in pH when small quantities of acid or base are added to them. They achieve this by containing both a weak acid and its conjugate base (or a weak base and its conjugate acid). The weak acid and its conjugate base react with the added acid or base, effectively neutralizing it and preventing a significant change in pH.
Let's use the example of adding NaOH to a solution of acetic acid (HAc) to form a buffer. Acetic acid is a weak acid that partially dissociates in water to produce acetate ions (Ac-) and hydrogen ions (H+). When NaOH, a strong base, is added to this solution, it reacts with the acetic acid to form water and sodium acetate. This reaction can be represented as follows:
HAc + NaOH -> H2O + NaAc
In this reaction, the strong base (NaOH) reacts with the weak acid (HAc) to form a salt (NaAc) and water, and the pH of the solution increases. However, the presence of both the weak acid (HAc) and its conjugate base (Ac-) allows the solution to act as a buffer. If a small quantity of acid or base is added, the buffer system will respond by consuming the added ions to maintain the equilibrium between the weak acid and its conjugate base. This prevents a significant change in pH.
When a small quantity of a strong acid is added to a buffer solution, the buffer will initially neutralize some of the added acid by reacting with it. As a result, the pH of the buffer solution will only change slightly. Similarly, when a small quantity of a strong base is added, the buffer will neutralize some of the added base, again resulting in a minimal change in pH.
However, if a large quantity of acid or base is added to the buffer solution, the buffer may become overwhelmed and unable to neutralize all of the added ions. At this point, the pH of the buffer solution will start to change significantly as the excess acid or base begins to dominate the system. The buffer capacity, which is the ability of the buffer to resist changes in pH, is limited and can be exceeded when a large quantity of acid or base is added.
In summary, buffers behave by maintaining a relatively constant pH in the presence of small quantities of acid or base. They achieve this by containing both a weak acid and its conjugate base (or a weak base and its conjugate acid), which react with the added ions and prevent a significant change in pH. However, when a large quantity of acid or base is added, the buffer capacity is exceeded, and the pH of the buffer solution will start to change significantly.