how is a bronsted lowry base distinguished from an Arrhenius base? explain with example
Answers
An Arrhenius base is a molecule that when dissolved in water will break down to yield an OH- or hydroxide in solution. To recognize the Arrhenius base look for a molecule ending in OH, but not following CHx which refers to an alcohol.
Arrhenius base examples include:
Sodium hydroxide – NaOH
Potassium hydroxide – KOH
Magnesium hydroxide – Mg(OH)2
and so many more…
This is where we start to see the difference between the Bronsted-Lowry and Arrhenius definitions. While the Arrhenius base referred specifically to the hydroxide (OH-) ion, the Bronsted-Lowry base refers to any atom or ion capable of accepting or bonding to a free proton in solution.
Referring back to the HNO3 + NH3 reaction above, when ammonia picks up the free H+ it acts as a proton-acceptor. NH3 is the Bronsted-Lowry base in this example.
Additional examples include:
Methanol – CH3OH
Formaldehyde – H2CO
And even water – H2O
Hope it helps you.
Namaste.
Answer:
Bronsted Concept of Acids and Bases
An Arrhenius Acid is something that donates a proton to water, and Bronsted-Lowry Concept extends this to any substance, where an acid is a proton donor and a base is a proton acceptor
Ammonia is the Bronsted-Lowry base because it is the 'proton acceptor' - it accepts a hydrogen atom from water. On the other hand, water is the Bronsted-Lowry acid because it is the 'proton donor'.