calculate the hydronium ion concentration in an aqueous solution that contains 2.50x10^-6M in hydroxide solution

(H^+)(OH^-) = Kw = 1E-14

You know OH^-, solve for H^+.
NOTE: (H^+) = (H3O^+)

49.1

To calculate the hydronium ion concentration in an aqueous solution, we can use the equation for the ion product of water, which is equal to [H₃O⁺] [OH⁻] = 1.0 x 10⁻¹⁴ at 25°C.

Given that the hydroxide ion concentration is 2.50 x 10⁻⁶ M, we can substitute this value into the equation and solve for the hydronium ion concentration.

[H₃O⁺] [OH⁻] = 1.0 x 10⁻¹⁴

[H₃O⁺] = (1.0 x 10⁻¹⁴) / [OH⁻]

[H₃O⁺] = (1.0 x 10⁻¹⁴) / (2.50 x 10⁻⁶)

[H₃O⁺] = 4.0 x 10⁻⁹ M

Therefore, the hydronium ion concentration in the aqueous solution is 4.0 x 10⁻⁹ M.

To calculate the hydronium ion concentration in an aqueous solution, you need to use the concept of the ion product of water (Kw). The ion product of water is the product of the concentrations of hydronium ions (H3O+) and hydroxide ions (OH-) in water and is always equal to 1.0 x 10^-14 at 25°C.

The equation for the ion product of water is:

Kw = [H3O+][OH-] = 1.0 x 10^-14

Given that the solution is 2.50 x 10^-6 M in hydroxide ions ([OH-]), we can use the ion product of water to solve for the concentration of hydronium ions ([H3O+]).

First, rearrange the equation to solve for [H3O+]:

[H3O+] = Kw / [OH-]

Substituting the given values:

[H3O+] = (1.0 x 10^-14) / (2.50 x 10^-6)

Calculating this expression:

[H3O+] ≈ 4.0 x 10^-9 M

Therefore, the hydronium ion concentration in the aqueous solution is approximately 4.0 x 10^-9 M.