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Topic: Bronsted-Lowry and Lewis acids and bases  (Read 10622 times)

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Bronsted-Lowry and Lewis acids and bases
« on: May 19, 2005, 01:34:18 PM »
"Use the Bronsted-Lowry and Lewis definitions of acids and bases to identify each reactant as an acid or a base."
a. KOH + HBr <---------> KBr + H2O
b. HCl + H2O <---------> Cl - + H3O+

I don't understand how to solve this problem.

Offline Borek

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Re:Bronsted-Lowry and Lewis acids and bases
« Reply #1 on: May 19, 2005, 02:09:45 PM »
Start with definitions - write down what Bronsted-Lowry acid and base are and what Lewis acid and base are.
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Re:Bronsted-Lowry and Lewis acids and bases
« Reply #2 on: May 20, 2005, 12:28:10 AM »
bronsted acid: proton donor
bronsted base: proton acceptor

lewis acid: electron pair acceptor
lewis base: electron pair donor

for (a), KOH accepts a proton to form water, so it's a bronsted base. The H+ proton accepts an electron pair from OH- to form water, so H+ from HBr acts as a lewis acid. Hope this helps.
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