What is the pH of a 0.0344 M KOH solution?
Here's what I have done...
[OH] = 0.0344
pOH = -log(0.0344)
= 1.463
pH + pOH = 14.0
pH + (1.463) = 14.0
pH = 12.537
Is this correct?
yes.
Well, the pH of a 0.0344 M KOH solution is not a joke at all! It's actually quite basic... literally! You see, KOH is a strong base, and when it dissolves in water, it completely dissociates into hydroxide ions (OH-). So, in this case, your solution would be very alkaline, with a high pH value. If you really want to know the exact pH, you'd have to perform a calculation using the concentration, but one thing is for sure: it won't be anywhere near clown-normal!
To find the pH of a solution, we need to determine the concentration of hydrogen ions (H+) in the solution.
For a base, like KOH, we know that it dissociates in water to form hydroxide ions (OH-).
The dissociation equation for KOH is:
KOH -> K+ + OH-
Here, for every 1 molecule of KOH that dissolves, it produces 1 hydroxide ion (OH-).
Since the concentration of KOH is given as 0.0344 M, the concentration of hydroxide ions (OH-) in the solution is also 0.0344 M.
Now, we know that the concentration of hydrogen ions (H+) in any solution can be found using the expression Kw = [H+][OH-], where Kw is the ion product of water, equal to 1.0 x 10^-14.
Rearranging the equation, we have [H+] = Kw / [OH-].
Plugging in the values, we get:
[H+] = (1.0 x 10^-14) / (0.0344)
Calculating this, we find that [H+] = 2.91 x 10^-13 M.
Finally, to find the pH, we can use the formula:
pH = -log[H+]
Using this formula, we get:
pH = -log(2.91 x 10^-13)
Evaluating this expression, we find that the pH of the 0.0344 M KOH solution is approximately 12.54.
To determine the pH of a solution, we need to know the concentration of the hydrogen ion (H+). In this case, we have a solution of KOH, which is a strong base. In a strong base solution, all the KOH dissociates into its constituent ions, K+ and OH-. Since the hydroxide ion (OH-) is a strong base, it readily accepts a hydrogen ion to form water, so we can assume that OH- is equal to the concentration of H+ in this solution.
Given that the concentration of KOH is 0.0344 M, we can say that the concentration of OH- (and therefore H+) is also 0.0344 M.
Now, to calculate the pH, we need to take the negative logarithm (base 10) of the hydrogen ion concentration. Therefore, the formula for pH is:
pH = -log[H+]
Substituting the concentration of OH- (which is equal to H+), we have:
pH = -log[0.0344]
Using a scientific calculator, we can find that the pH of the given solution is approximately 1.46.