If the concentration of H3O+ is 3.5 X 10^-3 M. What is the concentration of OH-
(H^+)(OH^-) = Kw
Kw = 1 x 10^-14
To find the concentration of OH-, you can use the equation for the ion product of water (Kw):
Kw = [H3O+][OH-]
Since the concentration of H3O+ is given as 3.5 x 10^-3 M, and we know that water is neutral, we can assume that the concentration of OH- is the same (i.e., [OH-] = [H3O+]).
Substituting this information into the equation:
Kw = [H3O+][OH-]
Kw = (3.5 x 10^-3 M)(3.5 x 10^-3 M)
The value of the ion product of water, Kw, is 1.0 x 10^-14 at 25°C. Therefore, we can solve for [OH-]:
1.0 x 10^-14 = (3.5 x 10^-3 M)(3.5 x 10^-3 M)
Divide both sides of the equation by (3.5 x 10^-3 M):
[OH-] = (1.0 x 10^-14) / (3.5 x 10^-3 M)
Simplifying further:
[OH-] = 2.86 x 10^-12 M
Therefore, the concentration of OH- is approximately 2.86 x 10^-12 M.
To find the concentration of OH- (hydroxide ion), we can use the concept of Kw, which represents the equilibrium constant for the auto-ionization of water. The equation for this auto-ionization is:
H2O ⇌ H3O+ + OH-
At 25°C, Kw = 1.0 x 10^-14 M^2. This can be expressed as:
[H3O+] x [OH-] = Kw
Given that the concentration of H3O+ is 3.5 x 10^-3 M, you can substitute this value into the equation:
(3.5 x 10^-3 M) x [OH-] = 1.0 x 10^-14 M^2
Now, we can rearrange the equation to solve for [OH-]:
[OH-] = (1.0 x 10^-14 M^2) / (3.5 x 10^-3 M)
By calculating this expression, we find that the concentration of OH- is approximately 2.9 x 10^-12 M.