In a 1.0 x10-6 M of HNO3 (aq) at 25 degrees celsius identify the relative molar amounts of theses species
HNO3-
H3O+
OH-
NO3-
H2O
What's HNO3-?
HNO3 must be zero
H2O must the the largest?
NO3^- must be 1E-6?
To determine the relative molar amounts of the species in a 1.0 x 10^-6 M HNO3 (aq) solution at 25 degrees Celsius, we need to consider the ionization of HNO3.
HNO3 is a strong acid, which means it will completely dissociate in water. The ionization of HNO3 can be represented as follows:
HNO3(aq) ↔ H+(aq) + NO3-(aq)
Since HNO3 is a strong acid, H+ and NO3- will be present in equal amounts. Therefore, the molar amounts of HNO3-, H3O+, OH-, NO3-, and H2O in the solution can be determined as follows:
HNO3-(aq): No dissociation occurs, so the molar amount is 0 (negligible).
H3O+(aq): Since HNO3 completely dissociates, the concentration of H+ (H3O+) is equal to the initial concentration of HNO3. Therefore, the molar amount of H3O+ is 1.0 x 10^-6 M.
OH-(aq): HNO3 is an acid, so it does not contribute OH- ions to the solution. Therefore, the molar amount of OH- is 0 (negligible).
NO3-(aq): Since HNO3 completely dissociates, the concentration of NO3- is equal to the initial concentration of HNO3. Therefore, the molar amount of NO3- is 1.0 x 10^-6 M.
H2O: H2O is the solvent in this case, so its molar amount is usually taken as the excess. Its molar amount is much larger compared to the other species present in the solution.
So, in summary, in a 1.0 x 10^-6 M HNO3 (aq) solution at 25 degrees Celsius, the relative molar amounts of the species are as follows:
HNO3-: Negligible (0)
H3O+: 1.0 x 10^-6 M
OH-: Negligible (0)
NO3-: 1.0 x 10^-6 M
H2O: Excess (compared to other species)