The [OH-] of a solution with a PH 5.75 is

is it 5.6*10-9M?

14-5.75= pOH

pOH=8.25

Since pOH=-log[OH-]

10^(-8.25)=OH-=5.62 x10^-9M

That's what I got.

Aww thanks soo much buddy :)

To find the concentration of hydroxide ions ([OH-]) in a solution given its pH, you can use the equation:

pOH = 14 - pH

First, let's calculate the pOH using the given pH:

pOH = 14 - 5.75
pOH = 8.25

Next, to find the concentration of hydroxide ions ([OH-]), we can use the equation:

[OH-] = 10^(-pOH)

Now, let's substitute the value of pOH into the equation:

[OH-] = 10^(-8.25)
[OH-] ≈ 5.62 × 10^(-9) M

So, the concentration of hydroxide ions ([OH-]) in the given solution is approximately 5.62 × 10^(-9) M. Therefore, the answer is close to 5.62 × 10^(-9) M, not exactly 5.6 × 10^(-9) M as you mentioned.