Write the formulas of the conjugate bases of the following Bronsted-Lowry acids?
Could someone please explain how to determine the conjugate bases of the following Brønsted-Lowry acids?
A. HCN
B. (CH3)2NH2+
C. H3PO4
D. HSeO3-
1 Answers
When you have a Bronsted acid, its typical reaction is to give up a proton, otherwise written as an H+ ion. Once the Brosted acid loses the proton, the new molecule is considered a Bronsted base, since it could accomodate a proton to return to its original state (Bronsted bases accept protons). Thus, your answers are simply the molecule minus an H+. Remember to take off a charge unit.
A. CN-
B. (CH3)2NH (there are many hydrogens here, but you only take off the most acidic one.
C. H2PO4-
D.SeO3 2- (that last 2 is part of the charge)
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