What is the pOH of a solution which has a [H+] = 1.0 × 10¯³M?
pH = -log(H^+). Then
pH + pOH = pKw = 14
Solve for pOH.
To find the pOH of a solution, you need to know the concentration of hydroxide ions ([OH-]). However, in the given question, the concentration of the hydrogen ions ([H+]) is provided. To find the pOH, we will first convert the [H+] to [OH-].
In a neutral solution, the product of [H+] and [OH-] is equal to 1.0 × 10^-14, as determined by the ion product constant for water (Kw).
[H+] × [OH-] = 1.0 × 10^-14
Since the concentration of hydroxide ions can be considered equal to [H+] in an acidic solution, we have:
[H+] × [H+] = 1.0 × 10^-14
Taking the square root of both sides gives:
[H+] = √(1.0 × 10^-14)
[H+] = 1.0 × 10^-7 M
Now that we have the concentration of hydroxide ions, we can find the pOH using the following equation:
pOH = -log[OH-]
Since [OH-] is equal to [H+] in an acidic solution, we can substitute [H+] into the equation:
pOH = -log[H+]
pOH = -log(1.0 × 10^-7)
Now, using a scientific calculator or a logarithm table, you can calculate the pOH value. The logarithm of 1.0 × 10^-7 is 7, so:
pOH ≈ -7
Therefore, the pOH of the solution is approximately -7.