What is the hydroxide ion concentration in a solution with [H3O-] = 7.67 x 10^-9M
To find the hydroxide ion concentration, we can start by using the equation for the concentration of water (H2O) dissociating into hydronium (H3O+) and hydroxide (OH-) ions:
H2O ⇌ H3O+ + OH-
At 25 degrees Celsius, the concentration of water can be approximated as 55.5 M.
Since the solution is neutral, the concentration of hydronium ions ([H3O+]) is equal to the concentration of hydroxide ions ([OH-]). Therefore, the hydroxide ion concentration is also 7.67 x 10^-9 M.
To find the hydroxide ion concentration in a solution, you can use the concept of the ion product of water, which is defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C.
In this case, you are given the concentration of [H3O-] as 7.67 x 10^-9 M. Since the product of [H3O+] and [OH-] is always equal to 1.0 x 10^-14, you can calculate the concentration of the hydroxide ion ([OH-]) using the given concentration of the hydronium ion ([H3O-]).
Here's how you can find the hydroxide ion concentration:
1. Start with the ion product of water equation: Kw = [H3O+][OH-] = 1.0 x 10^-14.
2. Substitute the given concentration of [H3O-]: 1.0 x 10^-14 = (7.67 x 10^-9)[OH-].
3. Rearrange the equation to solve for [OH-]: [OH-] = (1.0 x 10^-14) / (7.67 x 10^-9).
4. Calculate the value: [OH-] ≈ 1.3 x 10^-6 M.
Therefore, the hydroxide ion concentration in the solution is approximately 1.3 x 10^-6 M.