pka v. ka

Acidity
Basicity
The Conjugate Seesaw

Moderators: Chem_Mod, Chem_Admin

Abigail Menchaca_1H
Posts: 104
Joined: Sat Sep 07, 2019 12:19 am

pka v. ka

Postby Abigail Menchaca_1H » Sun Dec 01, 2019 11:18 pm

What is the difference between pKA and KA?

JasonKwon_3k
Posts: 51
Joined: Thu Jul 11, 2019 12:16 am

Re: pka v. ka

Postby JasonKwon_3k » Sun Dec 01, 2019 11:20 pm

pKa = -log(ka)

madawy
Posts: 81
Joined: Fri Aug 09, 2019 12:17 am

Re: pka v. ka

Postby madawy » Sun Dec 01, 2019 11:21 pm

Whenever you see a "p" in front of a value, like pH, pKa, and pKb, it means you're dealing with a -log of the value following the "p". For example, pKa is the -log of Ka. Because of the way the log function works, a smaller pKa means a larger Ka.

sbeall_1C
Posts: 109
Joined: Sat Sep 07, 2019 12:17 am
Been upvoted: 1 time

Re: pka v. ka

Postby sbeall_1C » Sun Dec 01, 2019 11:22 pm

The difference between pKa and Ka is that the pKa is the negative logarithm of Ka. The lower the Ka value, the greater the pKa value, and therefore the stronger the acid.

zoedfinch1K
Posts: 57
Joined: Thu Jul 25, 2019 12:16 am

Re: pka v. ka

Postby zoedfinch1K » Sun Dec 01, 2019 11:23 pm

KA is the equilibrium constant with the formula:
KA= [products]/[reactants]

pKA is just the -log of the KA:
pKA= -log[KA]


Return to “Acidity & Basicity Constants and The Conjugate Seesaw”

Who is online

Users browsing this forum: No registered users and 1 guest