If the hydronium ion concentration of a aqueous solution at 25 degrees celcius is 5*10^-6 M, what is the hydroxide ion concentration
To find the hydroxide ion concentration in the aqueous solution, you can use the equation for the self-ionization of water, which states that the product of the hydrogen ion concentration (H+) and the hydroxide ion concentration (OH-) is always equal to a constant value at a given temperature. This constant is known as the ion product of water (Kw).
The ion product of water (Kw) at 25 degrees Celsius is 1.0 x 10^-14 M^2. This means that the product of the hydrogen ion concentration and the hydroxide ion concentration in any aqueous solution at this temperature will always equal 1.0 x 10^-14 M^2.
Let's denote the hydroxide ion concentration as [OH-]. Since the hydronium ion concentration ([H3O+]) is given as 5 x 10^-6 M, we can calculate the hydroxide ion concentration ([OH-]) using the ion product of water equation:
[H3O+] x [OH-] = Kw
Substituting the known values:
(5 x 10^-6 M) x [OH-] = 1.0 x 10^-14 M^2
Solving for [OH-]:
[OH-] = (1.0 x 10^-14 M^2) / (5 x 10^-6 M)
[OH-] = 2.0 x 10^-9 M
Therefore, the hydroxide ion concentration in the aqueous solution is 2.0 x 10^-9 M.
To find the hydroxide ion concentration in an aqueous solution, you can use the concept of Kw, which represents the equilibrium constant for water dissociation. At 25 degrees Celsius, Kw is equal to 1.0 x 10^-14.
The relationship between hydronium ion (H3O+) concentration and hydroxide ion (OH-) concentration is governed by the following equation:
Kw = [H3O+][OH-]
Given that the hydronium ion concentration ([H3O+]) is 5 x 10^-6 M, we can rearrange the equation to solve for the hydroxide ion concentration ([OH-]):
[OH-] = Kw / [H3O+]
[OH-] = (1.0 x 10^-14) / (5 x 10^-6)
[OH-] = 2 x 10^-9 M
Therefore, the hydroxide ion concentration in the given aqueous solution is 2 x 10^-9 M.
Note that the correct spelling is celsius.
(H3O^+)(OH^-) = Kw = 1E-14.
You know H3O^+ and Kw, calculate OH^-.