Multiple Choice
Which of the following is a typical property of a base (in aqueous solution)?
35
views
17. Acid and Base Equilibrium
Bases
Multiple Choice
Which of the following is the weakest Brønsted–Lowry base in water?
A
B
C
D
Verified step by step guidance1
Recall that a Brønsted–Lowry base is a species that can accept a proton (H\(\textsuperscript{+}\)). The strength of a base in water is related to its tendency to accept a proton from water or other acids.
Identify the given bases: hydroxide ion (OH\(\textsuperscript{−}\)), methyl anion (CH\(\textsubscript{3}\[\textsuperscript{−}\)), fluoride ion (F\(\textsuperscript{−}\)), and amide ion (NH\(\textsubscript{2}\]\textsuperscript{−}\)).
Understand that the strength of these bases depends on the stability of their conjugate acids and the electronegativity of the atoms bearing the negative charge. More electronegative atoms stabilize the negative charge better, making the base weaker.
Compare the bases by considering the electronegativity of the atoms: fluorine is the most electronegative, followed by oxygen, nitrogen, and carbon. Therefore, fluoride ion (F\(\textsuperscript{−}\)) holds its negative charge more tightly and is less likely to accept a proton, making it the weakest base among the options.
Summarize that the weakest Brønsted–Lowry base in water is the one with the most stable conjugate acid and the highest electronegativity on the atom bearing the negative charge, which corresponds to F\(\textsuperscript{−}\).
Related Videos
Related Practice
