Question

If 0.016 mol of NaOH were added to 0.500 L of a sodium acetate-acetic acid buffer that contains 0.25 M NaC2H3O2 and 0.19 M HC2H3O2, by how many pH units will the pH of the buffer change?​

Answer 1

A buffer solution resists changes in pH when acid or base is added to it. The pH of a buffer is determined by the equilibrium between the weak acid and its conjugate base. To calculate the change in pH when NaOH is added to the buffer, we can use the Henderson-Hasselbalch equation.

Step-by-step explanation:

A buffer solution is a solution that resists changes in pH when acid or base is added to it. The pH of a buffer solution is determined by the equilibrium between the weak acid and its conjugate base. In this case, the NaC2H3O2 and HC2H3O2 are a conjugate acid-base pair.

To calculate the change in pH when NaOH is added to the buffer, we need to consider the reaction between NaOH and HC2H3O2. HC2H3O2 + NaOH -> NaC2H3O2 + H2O

We can use the Henderson-Hasselbalch equation to calculate the pH change: pH = pKa + log ([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid. Given the concentrations and volume of the buffer solution, we can calculate the initial pH and then use the Henderson-Hasselbalch equation to calculate the change in pH.