Acids and Base Equilibria

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AGaeta_2C
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Joined: Wed Sep 18, 2019 12:21 am

Acids and Base Equilibria

Postby AGaeta_2C » Tue Jan 14, 2020 9:40 pm

What is the difference between strong acids/bases and weak ones in terms of calculating K?

Ally Huang- 1F
Posts: 103
Joined: Thu Jul 25, 2019 12:16 am

Re: Acids and Base Equilibria

Postby Ally Huang- 1F » Tue Jan 14, 2020 9:46 pm

The equilibrium constants of strong acids and bases and weak acids and bases are calculated in the same way. It is still products over reactants and the products and reactants are raised to the power of their stoichiometric coefficient. Strong acids and bases will have a very large K value because there are way more products than reactants at equilibrium. Strong acids and bases usually fully dissociate. Weak acids and bases will have a small K because there are way more reactants than products at equilibrium.

Giselle Littleton 1F
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Joined: Wed Sep 18, 2019 12:20 am

Re: Acids and Base Equilibria

Postby Giselle Littleton 1F » Wed Jan 15, 2020 8:55 am

Additionlly, a strong acid wil have a small pKa value and a strong base will have a small pKb value.

Izzie Capra 2E
Posts: 103
Joined: Sat Sep 07, 2019 12:19 am

Re: Acids and Base Equilibria

Postby Izzie Capra 2E » Wed Jan 15, 2020 12:00 pm

Yes, and when working with weak acids and bases (Ka and Kb), you will most likely be working with an ICE table to determine concentrations and percent dissociation (since weak acids and bases don't fully dissociate in water).

Miriam Villarreal 1J
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Joined: Sat Aug 17, 2019 12:16 am

Re: Acids and Base Equilibria

Postby Miriam Villarreal 1J » Wed Jan 15, 2020 4:56 pm

Strong acids have a High KA, however a small pKA meaning it dissociate more in water. In contrast, a weak acid is less likely to ionize and release a hydrogen ion, thus resulting in a less acidic solution. The same goes for a strong base in which they will have a high KB but a small pKB.


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