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.