Which of the following substances can act as a Bronsted acid in aqueous solution? (Select all that apply.)
NH41+
H2
O2
C4H10
H2CO3
H2SO4
H3O1+
1 5 6 7
To determine which substances can act as a Bronsted acid in aqueous solution, we need to understand what a Bronsted acid is. In the Bronsted-Lowry theory of acids and bases, an acid is a substance that donates a proton (H+) to another substance.
Let's analyze each of the given substances to determine if it can act as a Bronsted acid:
1. NH4+ (ammonium ion): In aqueous solution, NH4+ can donate a proton (H+) to water, making it a Bronsted acid.
2. H2 (hydrogen gas): H2 does not contain any extra protons that it can donate in aqueous solution. Therefore, it cannot act as a Bronsted acid.
3. O2 (oxygen gas): O2 does not contain any protons and cannot donate any in aqueous solution. So, it cannot act as a Bronsted acid.
4. C4H10 (butane): Butane does not contain any protons that it can donate in aqueous solution. Hence, it cannot act as a Bronsted acid.
5. H2CO3 (carbonic acid): H2CO3 can donate two protons to water, making it a Bronsted acid. It can donate one proton to form HCO3- (bicarbonate ion) and another proton to form CO32- (carbonate ion).
6. H2SO4 (sulfuric acid): H2SO4 can donate two protons to water, making it a strong Bronsted acid. It can donate one proton to form HSO4- (hydrogen sulfate ion) and another proton to form SO42- (sulfate ion).
7. H3O+ (hydronium ion): In aqueous solution, H3O+ acts as the main species involved in acid-base reactions. It readily donates a proton (H+) to other substances, making it a Bronsted acid.
So, the substances that can act as Bronsted acids in aqueous solution are: NH4+, H2CO3, H2SO4, and H3O+.