What are Bronsted acids and bases?
A Brønsted-Lowry acid is any substance (molecule or ion) that can donate a hydrogen ion (
A Brønsted-Lowry base is any species that can accept a hydrogen ion (
In short, acids are proton donors and bases are proton acceptors.
Take the following reaction for example:
Hydrochloric acid ( The Brønsted-Lowry theory also introduces the concept of conjugate acid-base pairs. A conjugate acid-base pair are two species that differ by a ( Based on the reaction above, the ammonium ion Here's a tip to let you know which substance is the conjugate acid and which substance is the conjugate base: A conjugate base has one less ( A conjugate acid has one more ( Here's a general depiction of conjugate acid-base pairs:
I really hope this makes sense!
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Bronsted acids are proton donors, meaning they can donate a proton (H⁺). Bronsted bases are proton acceptors, meaning they can accept a proton.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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