Give the conjugate base of the following Bronsted-Lowry acids. (Type your answer using the format CO2 for CO2, [H2AsO4]- for H2AsO4-, and [Ni(CN)4]2- for Ni(CN)42-.)
1) H2SO4
I have tried H[SO4]- and just HSO4 but they are both wrong:(
If I understand the directions given, I would type in [HSO4]- since
H2SO4 ==> H^+ + HSO4^-
To find the conjugate base of H2SO4, you need to remove one proton (H+) from the acid.
H2SO4 can lose one proton to form the conjugate base.
The correct answer is [HSO4]-.
To determine the conjugate base of an acid, you need to remove a proton (H+) from the acid molecule. In the case of H2SO4, it is a strong acid that can easily donate two protons.
To find the conjugate base, you need to remove one proton, leaving behind the remaining species. Let's follow the steps:
Step 1: Identify the acid - H2SO4
Step 2: Remove one proton (H+) from the acid molecule
Step 3: The remaining species after removing the proton is the conjugate base
In this case, removing one proton from H2SO4, we get [HSO4]- as the conjugate base. However, you mentioned that it was marked incorrect.
It is possible that the answer they are looking for is the fully deprotonated form of sulfuric acid. In this case, we need to remove both protons. Let's follow the steps again:
Step 1: Identify the acid - H2SO4
Step 2: Remove both protons (H+) from the acid molecule
Step 3: The remaining species after removing the protons is the conjugate base
Removing both protons from H2SO4, we get [SO4]2- as the fully deprotonated conjugate base.
So, the possible answers for the conjugate base of H2SO4 can be [HSO4]- or [SO4]2-.