The reaction:
H2PO4- + HAsO42 ---> HPO4- + H2AsO4-
Which one of the sets above lists both of the base species involved in the equilibrium?
I'm confused and couldn't identify the conjugate acids and bases properly. Could Dr.Bob explain abt this problem ? Thank you
So,the answers are HAsO42- & HPO4- rite?
Because from what I found,HAs04 2- is weakly basic and HPO4 2- is a conjugate base. So the bases are these two species above. M I rite?
Ah, chemistry can be quite confusing at times, but don't worry, I'm here to help! Let's break it down:
In this reaction, we have two pairs of acids and bases:
1. H2PO4- (dihydrogen phosphate) is the acid and HPO4- (monohydrogen phosphate) is its conjugate base.
2. HAsO42- (tetraoxoarsenate) is the acid and H2AsO4- (dihydrogen arsenate) is its conjugate base.
So, the base species involved in the equilibrium are HPO4- (monohydrogen phosphate) and H2AsO4- (dihydrogen arsenate).
Hope that clarifies things for you! If you have any more questions, feel free to ask.
In order to determine the conjugate acids and bases in this reaction, let's break it down step by step:
1. H2PO4- + HAsO42- ⇌ HPO4- + H2AsO4-
The H2PO4- molecule donates a proton (H+) to form the HPO4- molecule. Therefore, H2PO4- is acting as an acid in this reaction.
Conversely, HPO4- accepts a proton (H+) to form the H2PO4- molecule. Therefore, HPO4- is acting as a base in this reaction.
Similarly, HAsO42- donates a proton (H+) to form the H2AsO4- molecule, making HAsO42- the acid.
H2AsO4- accepts a proton (H+) to form the HAsO42- molecule, making H2AsO4- the base.
So, the acid-base pairs in this reaction are:
- Acid: H2PO4-
- Base: HPO4-
and
- Acid: HAsO42-
- Base: H2AsO4-
Sure! I can definitely help explain this problem. In order to identify the base species involved in the equilibrium, we need to understand the concept of conjugate acids and bases.
In a chemical reaction, an acid is a substance that donates a proton (H+), while a base is a substance that accepts a proton. When an acid loses a proton, it forms its conjugate base, and when a base accepts a proton, it forms its conjugate acid.
Looking at the given reaction:
H2PO4- + HAsO42- ---> HPO4- + H2AsO4-
To determine the base species involved in the equilibrium, we need to identify the substances that can accept a proton. In this reaction, H2PO4- can donate a proton and is therefore an acid, which means HPO4- is its conjugate base. Similarly, HAsO42- can also donate a proton and is an acid, which means H2AsO4- is its conjugate base.
So, in the given reaction, the base species involved are HPO4- (conjugate base of H2PO4-) and H2AsO4- (conjugate base of HAsO42-).
Therefore, the correct answer would be:
HPO4- and H2AsO4-
Acids give away H^+. Bases add them. Look for the one that give them away and accepts them.
H2PO4^- on the left and HPO4^2- on the right must be one pair. H2PO4^-has given one H away to something.
HAsO4^2- and H2AsO4^- must be the other pair.
So H2PO4^- has given a H to HAsO4^2-. In the process, H2PO4^- becomes HPO4^2- and HAsO4^2- becomes H2AsO4^-. It isn't that complicated. Just follow the H. It's easy to see which is missing and which has been added.