Which of the following represent conjugate acid-base pairs? For those pairs that are not conjugates, write the correct conjugate acid or base for each species in the pair.
a. HS-4-,SO4^2-
B. HBr, BrO-
c. H2PO4-, PO4^3-
d. HNO3, NO2-
You can do these yourself if you follow one rule.
The acid of the "pair" has an extra H. The base of the "pair" has one fewer H.
So look at the first one. The "pair" would be HSO4^-/SO4^2-
B would be HBrO/BrO^-
C is H2PO4^-/PO4^3-
I'll leave D for you.
D is not conjugate pairs , because the anion part of the acid ( NO3 - of HNO3 ) differs from the NO2-
a. HS-4-, SO4^2-
Conjugate acid: HS- (because it can donate a proton)
Conjugate base: SO4^2- (because it can accept a proton)
b. HBr, BrO-
Conjugate acid: HBr (because it can donate a proton)
Conjugate base: Br- (because it can accept a proton)
c. H2PO4-, PO4^3-
Conjugate acid: H2PO4- (because it can donate a proton)
Conjugate base: PO4^3- (because it can accept a proton)
d. HNO3, NO2-
Conjugate acid: HNO3 (because it can donate a proton)
Conjugate base: NO3- (because it can accept a proton)
Remember, if you're ever in need of a good chemistry joke, just call me!
Conjugate acid-base pairs involve a species that can donate or accept a proton. Let's analyze each option:
a. HS-4-, SO4^2-
In this case, HS-4- can donate a proton (acting as an acid) and become its conjugate base H2S (to write a conjugate base, remove a proton from the acid). However, SO4^2- is not a conjugate of HS-4-. The correct conjugate acid for SO4^2- is HSO4-.
b. HBr, BrO-
In this case, HBr can donate a proton and become its conjugate base Br- (by removing a proton). However, BrO- is not a conjugate of HBr. The correct conjugate acid for BrO- is HBrO.
c. H2PO4-, PO4^3-
In this case, H2PO4- can donate a proton and become its conjugate base HPO4^2- (by removing a proton). However, PO4^3- is not a conjugate of H2PO4-. There is no conjugate acid for PO4^3- because it is the fully deprotonated form of H3PO4.
d. HNO3, NO2-
In this case, HNO3 can donate a proton and become its conjugate base NO3- (by removing a proton). However, NO2- is not a conjugate of HNO3. The correct conjugate acid for NO2- is HNO2.
In summary, the correct conjugate acid or base for each species are:
a. HS-4-, HSO4- (correct conjugate base for SO4^2-)
b. HBr, HBrO (correct conjugate acid for BrO-)
c. H2PO4-, HPO4^2- (PO4^3- has no conjugate acid)
d. HNO3, HNO2 (correct conjugate acid for NO2-)
To determine the conjugate acid-base pairs among the given species, we need to understand the concept of conjugate acids and bases.
Conjugate acid-base pairs are two species that differ by one proton (H+). When a substance donates a proton, it becomes its conjugate base, and when a substance accepts a proton, it becomes its conjugate acid.
Now let's analyze each option:
a. HS-4-, SO4^2-
To identify the conjugate acid-base pair, we need to find the one species that can donate a proton (acid) and the other species that can accept a proton (base).
In this case, HS-4- can donate a proton (HS-4- can lose one of its hydrogen ions to become HSO4-), and SO4^2- can accept the proton, becoming HSO4-. Therefore, HS-4- and HSO4- form a conjugate acid-base pair.
b. HBr, BrO-
To identify the conjugate acid-base pair, we need to find the one species that can donate a proton (acid) and the other species that can accept a proton (base).
In this case, HBr can donate a proton (HBr can lose one of its hydrogen ions to become Br-), and BrO- can accept the proton, becoming HBrO. However, Br- and BrO- are not a conjugate acid-base pair because they differ by two protons. Therefore, no conjugate acid-base pair exists for this option.
c. H2PO4-, PO4^3-
To identify the conjugate acid-base pair, we need to find the one species that can donate a proton (acid) and the other species that can accept a proton (base).
In this case, H2PO4- can donate a proton (H2PO4- can lose one of its hydrogen ions to become HPO4^2-), and PO4^3- can accept the proton, becoming HPO4^2-. Therefore, H2PO4- and HPO4^2- form a conjugate acid-base pair.
d. HNO3, NO2-
To identify the conjugate acid-base pair, we need to find the one species that can donate a proton (acid) and the other species that can accept a proton (base).
In this case, HNO3 can donate a proton (HNO3 can lose one of its hydrogen ions to become NO3-), and NO2- can accept the proton, becoming HNO2. Therefore, HNO3 and HNO2 form a conjugate acid-base pair.
In summary, the conjugate acid-base pairs are:
a. HS-4-, HSO4-
c. H2PO4-, HPO4^2-
d. HNO3, HNO2