What is the [H3O+] of a solution with [OH-] = 6.3 × 10-4 M?
A. 6.3 × 10-18 M
B. 10.80 M
C. 6.3 × 10-4 M
D. 1.6 × 10-11 M
DrBob222 can you help me with this question please?
[OH-] [H+]=1E-14
[H+]=1E-14 /6.3E-4= ?
answer D is the closest
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Yes, I can help you with this question. To determine the [H3O+] concentration of a solution, you can use the equation for the ion product of water (Kw).
Kw = [H3O+][OH-]
At 25 degrees Celsius, Kw is equal to 1.0 x 10^-14, which means that the product of [H3O+] and [OH-] must equal 1.0 x 10^-14 for any aqueous solution.
In this case, you're given that [OH-] = 6.3 x 10^-4 M. We can use this information to calculate the [H3O+] concentration.
First, let's rearrange the equation to solve for [H3O+]:
[H3O+] = Kw / [OH-]
Plugging in the given values:
[H3O+] = (1.0 x 10^-14) / (6.3 x 10^-4)
Calculating this expression will give us the answer.
To find the concentration of [H3O+], you can use the equation Kw = [H3O+][OH-]. Kw is the ion product constant for water and is equal to 1.0 x 10^(-14) at 25 degrees Celsius.
Given that [OH-] is 6.3 x 10^(-4) M, we can substitute this value into the equation:
1.0 x 10^(-14) = [H3O+][6.3 x 10^(-4)]
Now, solve for [H3O+]:
[H3O+] = (1.0 x 10^(-14)) / (6.3 x 10^(-4))
[H3O+] = 1.6 x 10^(-11)
Therefore, the [H3O+] of the solution is 1.6 x 10^(-11) M.
The correct answer is D. 1.6 x 10^(-11) M.