Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: FouRRaW on June 01, 2006, 10:07:59 PM
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I have a question in the textbook.
How do all negative ions act as bases??
Does anybody have a link to a site i could find the answer? Or a hint?
Thanks
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HSO4- would only act like a base depending on the pH of the solution. ;)
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Is that smartass response??
I really don't know actually.
Or is it a hint?
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It may also depend on which definition of base you mean....
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I gues it'd be the bronsted-lowry definition. A base is a molecule or ion that can accept a H+ proton.
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Cause i can't just say a negative ion acts as a base by accepting a H+ ion, can i?
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Is that smartass response??
Not that time.
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Whenever acids & bases are mentioned, they're usually the Bronsted-Lowry type (H+ donors & acceptors). You might also hear about Lewis acids & bases, which involve donors/acceptors of electrons instead of H+, but these will be refered to as "Lewis acids" or "Lewis bases" (or often in organic chemistry, "electrophiles" & "nucleophiles") rather than simply "acids" or "bases" (unless your chemistry teacher or textbook happens to be fiendishly ambiguous :P ).
Anions of strong acids--like HSO4-, Cl- & NO3---won't accept H+, at least not to any significant degree. So, not all negative ions will act as a (Bronsted-Lowry) base.
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at least not to any significant degree
This may be the sticking point for some people though ;)