Which statement best describes a Bronsted-Lowry base
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Answered by
3
Answer:
it must accept promets to from a conjugate acid
Answered by
2
Answer:
It must accept protons to form a conjugate acid.
Explanation:
- A Bronsted-Lowry acid is any species that is capable of donating a proton—H+
- A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the H+
- Water is amphoteric, which means it can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base.
- Strong acids and bases ionize completely in aqueous solution, while weak acids and bases ionize only partially.
- The conjugate base of a Bronsted-Lowry acid is the species formed after an acid donates a proton. The conjugate acid of a Bronsted-Lowry base is the species formed after a base accepts a proton.
- The two species in a conjugate acid-base pair have the same molecular formula except the acid has an extra H+ compared to the conjugate base.
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