pho What is the difference between a Bronsted-Lowry Base and an Arrhenius base?
ID: 887609 • Letter: P
Question
pho What is the difference between a Bronsted-Lowry Base and an Arrhenius base? What is the difference between a Bronsted-Lowry acid and an Arrhenius acid? Look up on line the Ka values for the first proton release for citric acid and ascorbic acid and state which is the stronger acid. What would happen to the carboxyl group (I) of ascorbic acid at pH 8.2? (hint: look up the pKa for COOH - it can vary somewhat, but that won't change the answer.)). The pH of a solution is 8. What is the pOH? What is the proton concentration? 6. Show ALL your work. Vou are in the lab needing to make a buffer that will be effective at holding the pH to 8.5. Will an acetate buffer be a good choice , why or why not? You will need to look up one piece of information to do this problem.Explanation / Answer
1.
Arrhenius definition of Base: An Arrhenius base is a substance that when added to water increases the concentration of OH1- ions present. NaOH is an example of an Arrhenius base
Bronsted-Lowry Definition of Base: a Bronsted-Lowry base is defined as anything that accepts H1+ ions.
This definition includes all Arrhenius bases but, it is a more general.
NOTE: Ahrrenius has a larger scope and includes many substances that will have a basic pH but will NOT free OH- ions
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