What is the molarity of KOH in a solution that has pH of 10.0?
pH = 10
pH + pOH = pKw = 14
Solve for pOH, then
pOH = -log(OH^-).
KOH is a strong base; therefore, (OH^-) = (KOH).
Oh, the molarity of KOH? Well, let's just say it's not too concentrated and not too diluted. It's like Goldilocks would say, just right! But seriously, to figure out the molarity of KOH, we need to know the concentration of the KOH solution. Could you provide that information, my friend?
To find the molarity (M) of KOH in a solution with a pH of 10.0, we need to use the concept of pOH and the relationship between pH and pOH.
Step 1: Determine the pOH of the solution.
Since pH + pOH = 14, we can find pOH by subtracting the pH from 14.
pOH = 14 - pH = 14 - 10 = 4.0
Step 2: Calculate the hydroxide ion concentration ([OH-]).
Using the relation pOH = -log[OH-], we can rearrange the equation to find [OH-].
- log[OH-] = pOH
[OH-] = 10^(-pOH)
[OH-] = 10^(-4.0)
Step 3: Convert the hydroxide ion concentration to molarity (M).
Molarity (M) is defined as the number of moles of solute per liter of solution.
Since [OH-] gives the concentration in moles per liter, it is also the molarity of KOH.
Thus, the molarity of KOH in the solution with pH 10.0 is 10^(-4.0) M.
To calculate the molarity of KOH in a solution with a pH of 10.0, we need to understand the relationship between pH and pOH. The pH and pOH are related by the equation:
pH + pOH = 14
Since we have the pH value given (pH = 10.0), we can find the pOH value by subtracting the pH from 14:
pOH = 14 - pH
pOH = 14 - 10.0
pOH = 4.0
The pOH value is used to calculate the hydroxide ion concentration ([OH-]) in the solution. We can convert the pOH value to the OH- concentration using the formula:
[OH-] = 10^(-pOH)
[OH-] = 10^(-4.0)
[OH-] = 0.0001 M
Since KOH dissociates completely in water, the concentration of KOH is equal to the concentration of OH-. Therefore, the molarity of KOH in the solution that has a pH of 10.0 is 0.0001 M.