is HSO4 a weak acid
HSO4- is a stronger acid than NH4+
HSO4 is Hydrogen Sulphate and an amphiprotic species. It is the conjugate base of H2SO4. H2SO4 is sulphuric acid, a very strong acid.
This dissociation is a two step process: NaHSO4 ---> Na+ + HSO4- HSO4- <---> H+ + SO42- (weak acid protolysis)
The conjugate acid of HSO4- is H2SO4. HSO4- is the conjugate base of H2SO4 because it can accept a proton (H+) to form the acid.
HSO4, the bisulfate ion is acidic.
HSO4- is a stronger acid than NH4+
HSO4 is Hydrogen Sulphate and an amphiprotic species. It is the conjugate base of H2SO4. H2SO4 is sulphuric acid, a very strong acid.
This dissociation is a two step process: NaHSO4 ---> Na+ + HSO4- HSO4- <---> H+ + SO42- (weak acid protolysis)
The conjugate acid of HSO4- is H2SO4. HSO4- is the conjugate base of H2SO4 because it can accept a proton (H+) to form the acid.
HSO4, the bisulfate ion is acidic.
The conjugate acid of SO4 2- is HSO4 -, also known as bisulfate or hydrogen sulfate. It is formed by adding a hydrogen ion to the sulfate ion.
HSO4 can act as a base by gaining a hydrogen ion to make H2SO4. HSO4 can act as an acid by losing a hydrogen ion to make SO4.
HSO4 is a weaker acid than H2SO4 because the presence of the additional hydrogen atom in H2SO4 makes it more likely to donate a proton, resulting in a stronger acid. HSO4, on the other hand, only has one acidic hydrogen atom, making it less likely to donate a proton and therefore weaker in acidity.
It is a strong acid only for the first hydrogen ion that is produced. (1) H2SO4 --> H+ + HSO4^- The remaining bisulfate ion, HSO4^-, is a weak acid and only partially dissociates. (2) HSO4^- <==> H+ + SO4^2- A misconception is that since sulfuric acid is a strong acid, that it dissociates like this: (3) H2SO4 --> 2H+ + SO4^2- That simply isn't the case except for extremely dilute solutions. As the concentration of the acid decreases, the acid behaves more and more like a strong diporotic acid. At "infinite dilution" it is accurate to write the dissociation as equation (3).
HSO4-
Sulfuric acid.
Weak acids only partially dissociate in water, meaning they release fewer hydrogen ions. Strong acids, on the other hand, completely dissociate to release all their hydrogen ions in solution. This difference in dissociation behavior contributes to variations in acidity levels between weak and strong acids.