What is the [H3O+] for a neutral solution at 50 degrees celsius?
I know that kw=[H3O+][OH-] but I am not sure what to do to get the H3O. The value I have for kw=5.76e-14 and I have the pH 6.62 but I do not know what the OH would be.
Chemistry(Please help, thank you) - DrBob222, Saturday, March 31, 2012 at 10:03pm
A neutral solution has H3O^+ = OH^- so if the pH = 6.62 then the pOH 6.62
pH = 6.62 = -log(H3O^+).
Solve for (H3O^+)
I don't know if I put this in my calculator correctly but I got -0.82 after taking the -log of 6.62.
Key in 6.62, change the sign to negative, then punch the 10x button. The screen should return 2.3988E-7 which rounds to 2.40E-7M = OH^- = H3O^+
Oh ok I got it now thank you.
To find the [H3O+] for a neutral solution at 50 degrees Celsius, you first need to determine the pOH.
Given that the pH is 6.62, the pOH can be calculated as follows:
pOH = 14 - pH
pOH = 14 - 6.62
pOH = 7.38
Since the solution is neutral, the [H3O+] is equal to the [OH-]. To find the [OH-], you can use the relationship between [H3O+] and [OH-] in water, which is governed by the ion product of water (Kw).
Kw = [H3O+][OH-]
Given that Kw = 5.76e-14, you can substitute the value of Kw and the [H3O+] as [OH-] into the equation:
5.76e-14 = [H3O+][H3O+]
Now, solve for [H3O+] by taking the square root of both sides of the equation:
[H3O+] = sqrt(5.76e-14)
Using a scientific calculator, you will find that [H3O+] ≈ 7.588e-8 M.
Therefore, the [H3O+] for a neutral solution at 50 degrees Celsius is approximately 7.588e-8 M.
To find the concentration of H3O+ in a neutral solution at 50 degrees Celsius, you can use the equation Kw = [H3O+][OH-]. Since the solution is neutral, the concentrations of H3O+ and OH- are equal.
You have the value of Kw, which is 5.76e-14. To find the concentration of H3O+, you need to take the square root of Kw.
√(5.76e-14) = 2.40e-7
So the concentration of H3O+ in a neutral solution at 50 degrees Celsius is 2.40e-7 M.