Final answer:
The false statement regarding a solution of 1.0 M HNO3 is 'e. Kb [NO3-] < 0', as the base dissociation constant (Kb) can never be less than zero and NO3- does not accept protons in water.
Step-by-step explanation:
The question asks which statement is false regarding a solution of 1.0 M HNO3. To answer this question, we need to analyze each statement:
- a. pH = 0: This is true for a 1.0 M solution of a strong acid like HNO3.
- b. Ka [HNO3] > 0: This is true because the acid dissociation constant (Ka) for a strong acid is always greater than zero.
- c. [H+] = 1.0 M: This is true as HNO3 completely dissociates in water.
- d. [H+] > 10^-7 M > [OH-]: This is true because a solution of HNO3 is acidic and thus [H+] would be greater than 10^-7 M, making the solution acidic.
- e. Kb [NO3-] < 0: This statement is false. Kb is the base dissociation constant, and it can never be less than zero. The anion NO3- does not have a Kb because it is the conjugate base of a strong acid and does not accept protons in water.
Therefore, the false statement regarding a solution of 1.0 M HNO3 is e. Kb [NO3-] < 0.