A buffer mixture of acetic acid and potassium acetate has PH=5.24. The ratio of [CH3COO-]/[CH3COOH] in this buffer is, (pKa=4.74)

To solve this problem, we can use the Henderson-Hasselbalch equation, which is:

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

where:

• pH is the pH of the solution,
• pKa is the acid dissociation constant,
• [A-] is the concentration of the base (in this case, CH3COO-),
• [HA] is the concentration of the acid (in this case, CH3COOH).

Given in the problem, we have pH = 5.24 and pKa = 4.74. We can plug these values into the equation and solve for the ratio [A-]/[HA]:

5.24 = 4.74 + log([CH3COO-]/[CH3COOH])

Subtract 4.74 from both sides:

0.5 = log([CH3COO-]/[CH3COOH])

To remove the logarithm, we can use the property of logarithms that says that log base 10 of a number is the exponent to which 10 must be raised to get that number. So:

10^0.5 = [CH3COO-]/[CH3COOH]

Therefore, the ratio of [CH3COO-] to [CH3COOH] in this buffer is approximately 3.16.