What are the (a) [H+], (b) [OH-], (c) pH, and (d) pOH of a 0.002 M solution of HNO3?
To find the values of (a) [H+], (b) [OH-], (c) pH, and (d) pOH of a 0.002 M solution of HNO3, we need to understand the properties of the acid, HNO3.
HNO3 is a strong acid, which means it dissociates completely in water. When it dissolves in water, it ionizes to produce one hydronium ion (H+) and one nitrate ion (NO3-).
(a) [H+]: In a 0.002 M solution of HNO3, the concentration of hydronium ions ([H+]) is equal to the concentration of HNO3, which is 0.002 M.
(b) [OH-]: Since HNO3 is an acid, it produces hydronium ions (H+). Therefore, the concentration of hydroxide ions ([OH-]) would be negligible in this case. We can assume it to be 0 M for a strong acid.
(c) pH: The pH of a solution is determined by the concentration of hydronium ions ([H+]). We can calculate the pH using the formula: pH = -log [H+].
In this case, the concentration of hydronium ions ([H+]) is 0.002 M. Therefore, we can calculate the pH as follows:
pH = -log (0.002)
Using a calculator, we find that the pH is approximately 2.70.
(d) pOH: The pOH of a solution can be calculated using the formula: pOH = -log [OH-].
In this case, since the concentration of hydroxide ions ([OH-]) is assumed to be negligible (0 M), the pOH would be 0.
So, (a) [H+] = 0.002 M, (b) [OH-] = 0 M, (c) pH ≈ 2.70, and (d) pOH = 0.