Calculate the hydroxide ion of a solution of almond extracted of PH 3.8
pH + pOH = pKw = 14.
You know pH and pKw, solve for pOH.
Then pOH = -log(OH^-)
To calculate the hydroxide ion concentration of a solution, we can use the pH value and the equation Kw = [H+][OH-], where Kw is the ion product constant for water.
First, we need to convert the pH value to the hydrogen ion concentration ([H+]) using the equation:
[H+] = 10^(-pH)
In this case, the pH of the almond extract solution is 3.8, so:
[H+] = 10^(-3.8)
Next, we can use the equation Kw = [H+][OH-] to find the hydroxide ion concentration ([OH-]).
Kw is a constant value at a given temperature (usually 25°C) and has a value of 1.0 x 10^-14.
Since we already know the value of [H+] from the previous step, we can rearrange the equation to solve for [OH-]:
[OH-] = Kw / [H+]
Substituting the values:
[OH-] = (1.0 x 10^-14) / [H+]
Now we can substitute the value of [H+] from the first step into this equation to calculate [OH-]:
[OH-] = (1.0 x 10^-14) / (10^(-3.8))
Now we can solve for [OH-] using a calculator:
[OH-] ≈ 1.58 x 10^(-11)
Therefore, the hydroxide ion concentration in the almond extract solution is approximately 1.58 x 10^-11 M.