Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 x 10-3 M in hydronium ion.
To calculate the hydroxide ion concentration in the solution, we can use the equation for the ion product of water (Kw):
Kw = [H3O+][OH-]
Where Kw is a constant equal to 1.0 x 10^-14 at 25°C, [H3O+] is the hydronium ion concentration, and [OH-] is the hydroxide ion concentration.
Given that [H3O+] = 3.50 x 10^-3 M, we can rearrange the equation to solve for [OH-]:
[OH-] = Kw / [H3O+]
Substituting the values, we get:
[OH-] = (1.0 x 10^-14) / (3.50 x 10^-3)
Simplifying the calculation:
[OH-] = 2.86 x 10^-12 M
Therefore, the hydroxide ion concentration in the aqueous solution is 2.86 x 10^-12 M.
To calculate the hydroxide ion concentration in an aqueous solution, you can use the concept of the ion-product constant of water, also known as Kw.
The ion-product constant of water, Kw, is the product of the concentrations of hydronium ions (H3O+) and hydroxide ions (OH-) in a water solution at a given temperature. At 25 degrees Celsius, the value of Kw is generally considered to be 1.0 x 10^-14.
The concentration of hydronium ions (H3O+) is given as 3.50 x 10^-3 M. Since the solution is neutral, the concentration of hydroxide ions (OH-) will be the same as the concentration of hydronium ions.
To calculate the hydroxide ion concentration, you can use the formula:
Kw = [H3O+][OH-]
Since the concentration of OH- is equal to the concentration of H3O+, you can substitute [OH-] with x, and [H3O+] with 3.50 x 10^-3:
(1.0 x 10^-14) = (3.50 x 10^-3)(x)
Now, solve for x:
x = (1.0 x 10^-14) / (3.50 x 10^-3)
x ≈ 2.86 x 10^-12 M
Therefore, the hydroxide ion concentration in the aqueous solution is approximately 2.86 x 10^-12 M.