HClO4 is a stronger proton donor than HNO3, but in water both acids appear to be
ID: 526869 • Letter: H
Question
HClO4 is a stronger proton donor than HNO3, but in water both acids appear to be of equal strength: they are both 100% ionized. Why is this so? What solvent property would be necessary in order to distinguish between the acidities of these Brønsted acids? Select all that apply.
a.Changing to a different solvent could not distinguish between the two acids.
b.A solvent that is a stronger proton acceptor than water would be needed to distinguish between the two acids.
c.Both of these acids are much stronger acids than water.
d.A solvent that is a weaker proton acceptor than water would be needed to distinguish between the two acids
Explanation / Answer
(d) A solvent that is a weaker proton acceptor than water would be needed to distinguish between the two acids.
Because to a weaker proton acceptor only the stronger acid can donate its proton effectively.
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