A solution has a hydroxide-ion concentration of 7.48X10-5 M. What is it's hydronium-ion centration?
I have no idea where to begin on this question...
(H3O^+)(OH^-) = Kw = 1E-14
You know Kw and you know OH^-, solve for H3O^+.
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To find the hydronium-ion concentration, we need to use the concept of the autoionization of water. In water, a small fraction of water molecules can spontaneously dissociate into hydronium ions (H3O+) and hydroxide ions (OH-). The concentration of hydronium ions and hydroxide ions in pure water at 25 degrees Celsius is equal to 1.0 x 10^-7 M.
The equation for the autoionization of water is:
H2O ⇌ H3O+ + OH-
It is important to note that water is considered a neutral molecule, and the concentrations of hydronium and hydroxide ions are equal in pure water. So, when we add an acid or a base to water, the hydronium and hydroxide ion concentrations change accordingly.
In this case, we have the concentration of hydroxide ions (OH-) as 7.48 x 10^-5 M. Since the concentration of hydroxide ions and hydronium ions in water is equal, we can assume that the concentration of hydronium ions (H3O+) is also 7.48 x 10^-5 M.
So, the hydronium-ion concentration of the solution is 7.48 x 10^-5 M.