Question #d6dd9

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Truong-Son N.
Mar 30, 2017

Because the charges of chloride and nitrate are #-1#. You cannot achieve an anion that has a zero charge.

Bisulfate is #"HSO"_4^(-)# and bicarbonate is #"HCO"_3^(-)#. However, nitrate is #"NO"_3^(-)#... if you add an #"H"^(+)# to convert it to its conjugate acid, all you get is a neutral (and STRONG) acid, #"HNO"_3#. "Binitrate", by its naming scheme, would in theory be negatively charged, but nitric acid is clearly neutral. Thus, "binitrate" cannot exist.

What is the conjugate acid of #"Cl"^(-)#? Is it also strong?

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