Final answer:
To calculate the pH, pOH, Ka, Kb, pKa, and pKb of a 0.082M solution of triethylamine, we need to use the Kb of triethylamine. The Kb value can be calculated by using the equation Kb = Kw/Ka, where Ka is the acid dissociation constant. From the Kb value, we can calculate the hydroxide ion concentration (OH-) and then use the equation pH = 14 - pOH to find the pH. Additionally, pKa and pKb can be calculated by taking the negative logarithm of Ka and Kb respectively.
Step-by-step explanation:
Triethylamine (C6H15N) acts as a weak base. To calculate the pH, we need to use the Kb value of triethylamine. Given that Ka + Kb = Kw (ion product of water), we can calculate Kb using the equation Kb = Kw/Ka. Assuming Ka = 1.8 x 10^-5, we can substitute the value into the equation to find Kb = 5.56 x 10^-10. To calculate the hydroxide ion concentration (OH-) from Kb, we use the equation OH- = sqrt(Kb * [triethylamine]). After calculating OH-, we can use the equation pH = 14 - pOH to find the pH.
Using the Ka and Kb values for triethylamine, we can also calculate pKa and pKb. pKa is the negative logarithm of the acid dissociation constant (Ka), and pKb is the negative logarithm of the base dissociation constant (Kb). By taking the negative logarithm of Ka and Kb respectively, we can obtain pKa and pKb.