An oxidation number
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The pH of the solution of the given acid is 3.099
Let HX be the weak acid:
HX ⇌ +
For which:
= [
][
] / [HX]
If lies in the range
we can assume that the equilibrium concentrations used in the expression are a good enough approximation to the initial concentrations.
Rearranging and taking negative logs of both sides gives:
pH =
a is the concentration of the acid.
= -log (2×
) = 5.69
pH =
pH = 3.099
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