In a 1.0x10^-6 M soltution of HNO3(aq), identify the relative molar amounts of these species.
H2O , HNO3, H3O+,NO3-, OH-
I answered this below.
1 H2O
2 H3O+
3 NO3-
4 OH-
5 HNO3
To identify the relative molar amounts of the species in a 1.0x10^-6 M solution of HNO3(aq), we need to understand the dissociation of the acid and the equilibrium in the solution.
HNO3(aq) is a strong acid. When it dissolves in water (H2O), it undergoes complete dissociation into H3O+ (hydronium ions) and NO3- (nitrate ions). The reaction can be represented as:
HNO3(aq) + H2O(l) -> H3O+(aq) + NO3-(aq)
Since HNO3 is a strong acid, it will completely dissociate, and the concentration of HNO3 will be equal to the concentration of H3O+ ions.
In this case, the concentration of HNO3 (and H3O+) is given as 1.0x10^-6 M. Therefore, the molar amounts of the species in this solution would be:
H2O: Since water does not dissociate in this reaction, the molar amount of water remains the same as the volume of the solution.
H2O: 1.0x10^-6 M (same as the concentration of HNO3 and H3O+)
HNO3: As mentioned before, the molar amount of HNO3 is equal to the molar amount of H3O+ ions.
HNO3: 1.0x10^-6 M
H3O+: The concentration of H3O+ is given as 1.0x10^-6 M.
H3O+: 1.0x10^-6 M
NO3-: The negative ion (NO3-) is formed as a result of the dissociation of HNO3. Since HNO3 completely dissociates, the concentration of NO3- will be the same as the concentration of HNO3 and H3O+.
NO3-: 1.0x10^-6 M
OH-: In an acidic solution like this, the concentration of hydroxide ions (OH-) is negligible.
OH-: Negligible concentration