Question

what is the final pH of a solution made by mixing 100 ml of 0.05M acetic acid and 100 ml of 0.1M sodium acetic? assuming pKa for acetic acid is 4.76.

Answer 1

The final pH of the solution made by mixing 100 ml of 0.05M acetic acid with 100 ml of 0.1M sodium acetate is approximately 5.061, calculated using the Henderson-Hasselbalch equation.

Step-by-step explanation:

The student is asking about the final pH of a buffer solution created by mixing 100 ml of 0.05M acetic acid with 100 ml of 0.1M sodium acetate. To calculate this, we have to use the Henderson-Hasselbalch equation, which is:

pH = pKa + log([A-]/[HA])

Since we're mixing equal volumes of two solutions, we can find the concentration of acetic acid ([HA]) and acetate ([A-]) after mixing:

• [HA] = (0.05M acetic acid * 100 ml) / 200 ml total volume = 0.025M
• [A-] = (0.1M sodium acetate * 100 ml) / 200 ml total volume = 0.05M

Substituting the values into the Henderson-Hasselbalch equation and the given pKa (4.76) for acetic acid:

pH = 4.76 + log(0.05 / 0.025)

pH = 4.76 + log(2)

pH = 4.76 + 0.3010

pH = 5.061

Therefore, the final pH of the solution is approximately 5.061.

Answer 2

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