alculate the H3O+ concentration present in water under the following conditions. Enter your answer in scientific notation.
a. [OH-] = 8.9 x 10-5 M
1.1E-10
b. [OH-] = 3.8 x 10-3 M
2.6E-12
c. [OH-] = 4.8 x 10-12 M
2.1E-3
To calculate the H3O+ concentration in water, we can use the relationship between the H3O+ and OH- concentrations. In a neutral solution, the H3O+ and OH- concentrations are equal, and this is known as the self-ionization constant of water.
The self-ionization constant of water, Kw, is given by the product of the H3O+ and OH- concentrations:
Kw = [H3O+][OH-]
At 25°C, Kw has a constant value of 1.0 x 10^-14.
Using this information, we can rearrange the equation to solve for the H3O+ concentration:
[H3O+] = Kw / [OH-]
a. [OH-] = 8.9 x 10^-5 M
Since Kw = 1.0 x 10^-14, we can substitute the values into the equation:
[H3O+] = (1.0 x 10^-14) / (8.9 x 10^-5)
[H3O+] = 1.1 x 10^-10 M
Therefore, the H3O+ concentration under these conditions is 1.1 x 10^-10 M.
b. [OH-] = 3.8 x 10^-3 M
[H3O+] = (1.0 x 10^-14) / (3.8 x 10^-3)
[H3O+] = 2.6 x 10^-12 M
The H3O+ concentration under these conditions is 2.6 x 10^-12 M.
c. [OH-] = 4.8 x 10^-12 M
[H3O+] = (1.0 x 10^-14) / (4.8 x 10^-12)
[H3O+] = 2.1 x 10^-3 M
The H3O+ concentration under these conditions is 2.1 x 10^-3 M.