Final answer:
To calculate the pKb of the butyrate ion, the conjugate base of butyric acid, we use the equation pKa + pKb = pKw, with pKa of butyric acid being 4.83. By rearranging the equation, we find that the pKb of the butyrate ion is 9.17, indicating it is a relatively weak base.
Step-by-step explanation:
Calculating the pKb for the Butyrate Ion
The question asks to calculate the pKb for the butyrate ion, which is the conjugate base of butyric acid. Butyric acid has a pKa of 4.83 at 25°C. To find the pKb of the butyrate ion, we can use the relationship pKa + pKb = pKw, where pKw is the ionic product of water at 25°C and is equal to 14.00.
The pKa of butyric acid is given as 4.83. Therefore, we can rearrange the equation to solve for pKb:
pKb = 14.00 - 4.83
pKb = 9.17
This pKb value represents the strength of the butyrate ion as a base. A higher pKb value corresponds to a weaker base, meaning that the butyrate ion is a relatively weak base.