How can you write a net ion equation and identify the conjugate acid/base pairs for these followings?
KNO3
Na2HPO4
NH4Br
KNO3 doesn't hydrolyze.
HPO42- + H2O ==> H3O+ + PO43-
Which gave away the H+? That is HPO43-.So that is the conjugate base and HPO41- is the acid. H2O accepted the H+ so it is the base and H3O+ is the conjugate acid.
We could write it another way.
HPO42- + HOH ==> H2PO4- + OH-
So the HPO42- is the base and HOH is the acid.
Which way does it actually go? You look up the K2 and K3.
The first reaction, which is an ionization equation, is k3 for H3PO4.
The second one, which is an hydrolysis, is K = Kw/k2
MH4+ + HOH ==> NH3 + H3O^+
To write a net ionic equation and identify the conjugate acid/base pairs, we first need to understand the concept of acids, bases, and their reactions.
In an acid-base reaction, an acid donates a proton (H+) to a base. The acid that donates the proton is called the "conjugate acid," and the base that accepts the proton is called the "conjugate base."
Now let's determine the acids and bases in the given compounds:
1. KNO3:
Looking at the compound, we have K+ and NO3-. In this case, there are no hydrogen ions (H+). Therefore, KNO3 does not involve any acid/base reactions and does not have any conjugate acid/base pairs.
2. Na2HPO4:
Examining the compound, we have Na2+ and HPO4^2-. The HPO4^2- ion has the ability to accept a proton (H+), making it a base. When it accepts a proton, it becomes H2PO4^- (dihydrogen phosphate). Therefore, HPO4^2- is the conjugate base, and H2PO4^- is the conjugate acid.
3. NH4Br:
In this compound, NH4+ can donate a proton (H+) and act as an acid. When it donates a proton, it becomes NH3 (ammonia). Therefore, NH4+ is the conjugate acid, and NH3 is the conjugate base.
To write a net ionic equation, we would need a reaction involving these compounds. Without any information about the reaction, we cannot provide a specific net ionic equation. However, now you have identified the conjugate acid/base pairs for each compound.