If the pH of a particular solution is 2.08, then the [OH -] must be:
pH + pOH = pKw = 14, then
pOH = -log(OH^-)
To determine the concentration of hydroxide ions ([OH-]) in a solution based on its pH value, we can use the equation:
pH + pOH = 14
Given that the pH of the solution is 2.08, we can calculate the pOH:
pH + pOH = 14
2.08 + pOH = 14
pOH = 14 - 2.08
pOH = 11.92
To convert pOH back to [OH-] concentration, we can use the following equation:
[OH-] = 10^(-pOH)
Substituting the value of pOH:
[OH-] = 10^(-11.92)
[OH-] ≈ 6.31 x 10^(-12) M
Therefore, the [OH-] concentration of the solution is approximately 6.31 x 10^(-12) M.
To determine the [OH-] (hydroxide ion concentration) from the pH of a solution, we need to use the concept of the pH scale.
The pH scale is a logarithmic scale used to represent the acidity or alkalinity of a solution. The pH scale ranges from 0 to 14, where a pH of 7 represents a neutral solution, pH less than 7 indicates an acidic solution, and pH greater than 7 indicates an alkaline (basic) solution.
The relationship between the pH and the [OH-] concentration is given by the equation:
pOH = 14 - pH
Where pOH is the negative logarithm (base 10) of the hydroxide ion concentration [OH-].
In this case, the given pH is 2.08. So, we can calculate the pOH as follows:
pOH = 14 - 2.08
pOH = 11.92
To find [OH-], we need to convert pOH back to OH- concentration:
[OH-] = 10^(-pOH)
[OH-] = 10^(-11.92)
[OH-] ≈ 6.31 x 10^(-12)