Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion (hint: use Kw, solve for [H+])Group of answer choices5.00 × 10-11 M4.00 × 10-9 M4.00 × 10-10 M4.00 × 10-11 M
Question
Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion (hint: use Kw, solve for [H+])Group of answer choices5.00 × 10-11 M4.00 × 10-9 M4.00 × 10-10 M4.00 × 10-11 M
Solution
To solve this problem, we need to use the ion product of water (Kw), which is a constant at a given temperature. At 25 degrees Celsius, Kw is equal to 1.0 x 10^-14.
The formula for Kw is [H+][OH-] = Kw.
We know the concentration of hydroxide ions [OH-] is 2.50 x 10^-4 M. We can substitute this value into the formula and solve for [H+], the hydronium ion concentration.
So, [H+][2.50 x 10^-4 M] = 1.0 x 10^-14.
To solve for [H+], we divide both sides of the equation by [2.50 x 10^-4 M]:
[H+] = (1.0 x 10^-14) / (2.50 x 10^-4 M) = 4.00 x 10^-11 M.
So, the hydronium ion concentration in the solution is 4.00 x 10^-11 M.
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