Today's lecture

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Matt Sanruk 2H
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Today's lecture

Postby Matt Sanruk 2H » Wed Jan 15, 2020 10:27 pm

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

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

Re: Today's lecture

Postby Abigail Sanders 1E » Wed Jan 15, 2020 10:32 pm

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
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Joined: Wed Sep 18, 2019 12:21 am

Re: Today's lecture

Postby Matt Sanruk 2H » Wed Jan 15, 2020 10:43 pm

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

Sanjana K - 2F
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Re: Today's lecture

Postby Sanjana K - 2F » Thu Jan 16, 2020 9:29 am

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
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Re: Today's lecture

Postby Sean Cheah 1E » Thu Jan 16, 2020 9:40 am

The Henderson-Hasselbalch equation states that . Use an ICE table to determine the concentrations of the conjugate acid-base pair.

Matt Sanruk 2H
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Re: Today's lecture

Postby Matt Sanruk 2H » Mon Jan 20, 2020 8:04 pm

Sean Cheah 1E wrote:The Henderson-Hasselbalch equation states that . Use an ICE table to determine the concentrations of the conjugate acid-base pair.

This equation looks like it is very useful! Thanks!


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