1) Give an example of a buffer solution?

2) Explain how the buffer solution named in 1) resists changes in pH when an acid or alkali is added to it.

Acetic Acid(HOAc) + Sodium Acetate(NaOAc) => common ion solution that inhibits changes in pH with addition of quantities of H^+ or OH^-. If H^+ is added to the buffer solution, the excess reacts with the OAc^- ion to form HOAc and consumes the excess H^+. If OH^- is added, the OH^- ions combine with H^+ forming water and consumes the excess OH^-.

1) A common example of a buffer solution is a mixture of acetic acid (CH3COOH) and sodium acetate (CH3COONa). This buffer solution is often used in laboratories and is known as an acetic acid-acetate buffer.

2) The buffer solution resists changes in pH by utilizing the principles of acid-base equilibrium. It consists of a weak acid and its conjugate base (or a weak base and its conjugate acid) that are capable of reacting with any added acid or alkali.

When an acid is added to the buffer solution, it reacts with the weak base component of the buffer, forming its conjugate acid. This reaction helps to neutralize the added acid and prevents a significant increase in the concentration of hydrogen ions (H+) in the solution, thereby resisting a drop in pH.

On the other hand, when an alkali (base) is added to the buffer solution, it reacts with the weak acid component of the buffer, forming its conjugate base. This reaction helps to neutralize the added alkali and prevents a significant decrease in the concentration of hydrogen ions (H+), again resisting a major change in pH.

In essence, the buffer solution maintains a stable pH due to the equilibrium between the weak acid and its conjugate base (or weak base and its conjugate acid). This balance ensures that any added acid or alkali is efficiently neutralized, minimizing changes in the hydrogen ion concentration and thus maintaining the buffer's resistance to pH fluctuations.