Final answer:
For a 0.09933 M HNO3 solution, the concentration of H3O+ is equivalent to the acid concentration (0.09933 M), leading to a pH of 1.003. The [OH-] is calculated using the ion-product constant for water and is approximately 1.007 × 10⁻¹³ M with a corresponding pOH of 12.997.
Step-by-step explanation:
We are dealing with a 0.09933 M HNO₃ solution, which is a strong acid and will dissociate completely in water to produce H₃O⁺ and NO₃⁻ ions. The concentration of H₃O⁺ will be the same as the initial concentration of the acid, so [H₃O⁺] = 0.09933 M. To calculate the pH, we take the negative logarithm (base 10) of the hydrogen ion concentration:
pH = -log(0.09933) = 1.003. Now, let's find the concentration of OH⁻ ions. Since H₃O⁺ and OH⁻ are inversely related by the equation Kw = [H₃O⁺][OH⁻], where Kw is the ion-product constant for water at 25 °C (1.0 × 10⁻¹⁴), we have [OH⁻] = Kw / [H₃O⁺] = 1.0 × 10⁻¹⁴ / 0.09933 M ≈ 1.007 × 10⁻¹³ M. The pOH can be calculated as pOH = -log([OH⁻]) = -log(1.007 × 10⁻¹³) ≈ 12.997. Final results are:
- pH = 1.003
- [H₃O⁺] = 0.09933 M
- [OH⁻] = 1.007 × 10⁻¹³ M
- pOH = 12.997