Find the pH of 1.0 x10-8 M KOH solution

I tried to find it but i got 6 and that's acidic not basic.

I would do it this way.

pOH = -log(OH^-) = 8
pH + pOH = pKw = 14
pH = 14- pOH = 14-8 = 6
So what's wrong with 6? Your problem is that you failed to realize that since 7 is neutral where (H^+) = (OH^-) = 10^-7M each, so when OH^- is 1E-8 (NOTE THIS IS LESS THAN 10^-7) SO IT'S A WEAKER BASE WHICH MAKES IT A STRONGER ACID and that's what pH 6 is; i.e., an acid solution.
OR another way.
(H^+)(OH^-) = Kw = 1E-14
when x*y = constant
if y is down then x must be up

To determine the pH of a solution, we need to calculate the concentration of the hydronium ion (H3O+), which is equivalent to finding the negative logarithm of the hydrogen ion concentration (pH = -log[H+]).

In the case of a strong base like KOH, it dissociates completely in water to form potassium (K+) and hydroxide (OH-) ions. The concentration of hydroxide ions in the solution can be used to calculate the concentration of hydrogen ions.

The concentration of hydroxide ions (OH-) in the solution is given as 1.0 x 10^-8 M.

Since the concentration of OH- ions and H+ ions in a solution are related by the equation:

[H+] x [OH-] = Kw,

where Kw is the ion product of water, which is typically equal to 1.0 x 10^-14 at 25°C.

Rearranging the equation to solve for [H+], we get:

[H+] = Kw / [OH-],

[H+] = (1.0 x 10^-14) / (1.0 x 10^-8),

[H+] = 1.0 x 10^-6 M.

Now, we can find the pH using the equation pH = -log[H+]:

pH = -log(1.0 x 10^-6),

pH = 6.

Therefore, the pH of a 1.0 x 10^-8 M KOH solution is 6, indicating that it is slightly acidic. However, it is important to note that KOH is a strong base, so the pH of the solution depends on how much base is added to the water.

To find the pH of a solution, you can use the formula:

pH = -log[H+]

In this case, you are given the concentration of the hydroxide ion (OH-) in a solution, which is KOH (potassium hydroxide). To find the concentration of H+ ions, you need to use the dissociation reaction of water:

H2O ⇌ H+ + OH-

Since KOH is a strong base, it completely dissociates in water, meaning there is an equal amount of OH- ions as the concentration of KOH you were given. Therefore, the concentration of H+ ions will be equal to the concentration of OH- ions:

[H+] = [OH-] = 1.0 x 10^-8 M

Now, plug this concentration into the pH formula:

pH = -log(1.0 x 10^-8)

Using a scientific calculator or an online tool, perform the calculations:

pH = -log(1.0) + log(10^8)
pH = -1 + 8
pH = 7

Therefore, the pH of a 1.0 x 10^-8 M KOH solution is 7, which indicates it is neutral, not acidic or basic. It is important to note that the pH scale ranges from 0 to 14, where values below 7 are considered acidic, values above 7 are considered basic, and a pH of 7 is neutral.