## Today's lecture

Matt Sanruk 2H
Posts: 131
Joined: Wed Sep 18, 2019 12:21 am

### Today's lecture

So as long as we are given the Ka or Kb value, we can find the pH or pOH?

Abigail Sanders 1E
Posts: 112
Joined: Wed Sep 11, 2019 12:16 am

### Re: Today's lecture

I believe if you are given a pKa value you will have to use the concentration of H3O+ from that pKa equation to find the pH of the solution. Like if pKa=[H3O+][CH3COO-]/[CH3COOH]=2X10^-5 then you would have to know the other concentrations in the reaction to be able to find the concentration of H3O+ and thus the pH of the solution.

Matt Sanruk 2H
Posts: 131
Joined: Wed Sep 18, 2019 12:21 am

### Re: Today's lecture

Wouldn't pKa give an integer thats less than 7?

Sanjana K - 2F
Posts: 102
Joined: Sat Sep 07, 2019 12:17 am
Been upvoted: 1 time

### Re: Today's lecture

pKa is dependent on Ka so if the Ka is greater than 10^-7, then the pKa would be less than 7 but if Ka is less than 10^-7, then the pKa would be greater than 7.
Matt Sanruk 2H wrote:Wouldn't pKa give an integer thats less than 7?

Sean Cheah 1E
Posts: 105
Joined: Wed Sep 18, 2019 12:20 am

### Re: Today's lecture

The Henderson-Hasselbalch equation states that $pH = pK_{a} + log(\frac{[A^{-}]}{[HA]})$. Use an ICE table to determine the concentrations of the conjugate acid-base pair.

Matt Sanruk 2H
Posts: 131
Joined: Wed Sep 18, 2019 12:21 am

### Re: Today's lecture

Sean Cheah 1E wrote:The Henderson-Hasselbalch equation states that $pH = pK_{a} + log(\frac{[A^{-}]}{[HA]})$. Use an ICE table to determine the concentrations of the conjugate acid-base pair.

This equation looks like it is very useful! Thanks!