Textbook Question
Aqueous solutions of hydrogen sulfide contain H2S, HS-, S2-, H3O+ , OH-, and H2O in varying concentrations. Which of these species can act only as an acid? Which can act only as a base? Which can act both as an acid and as a base?
17. Acid and Base Equilibrium
Amphoteric Species
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following species is amphiprotic within an aqueous solvent?
a) Br– b) HC2H3O2 c) SO42– d) HSe– e) H3O+
A
Br–
B
HC2H3O2
C
SO42–
D
HSe–
E
H3O+
Verified step by step guidance1
Understand the concept of amphiprotic species: An amphiprotic species is one that can both donate and accept a proton (H+). This means it can act as both an acid and a base.
Analyze each option to determine if it can donate and accept a proton: a) Br– is a bromide ion and cannot donate a proton, so it is not amphiprotic. b) HC2H3O2 is acetic acid, which can donate a proton but not accept one, so it is not amphiprotic.
Continue analyzing: c) SO42– is a sulfate ion, which cannot donate a proton, so it is not amphiprotic. d) HSe– is a hydrogen selenide ion, which can donate a proton to form Se2– and accept a proton to form H2Se, making it amphiprotic.
Evaluate the last option: e) H3O+ is the hydronium ion, which can donate a proton to form H2O but cannot accept another proton, so it is not amphiprotic.
Conclude that the species HSe– is the only one that can both donate and accept a proton, making it amphiprotic in an aqueous solution.
Related Videos
Related Practice
Amphoteric Species practice set
Problem sets built by lead tutorsExpert video explanations