Question #5cf09
1 Answer
Here's what I got.
Explanation:
Acetic acid is a weak acid, which means that an ionization equilibrium exists in aqueous solutions of acetic acid
#"CH"_ 3"COOH"_ ((aq)) + "H"_ 2"O"_ ((l)) rightleftharpoons "CH"_ 3"COO"_ ((aq))^(-) + "H"_ 3"O"_ ((aq))^(+)#
Notice that every mole of acetic acid that ionizes in solution produces
This implies that the equilibrium concentrations of the two ions will be equal.
#["CH"_3"COO"^(-)] = ["H"_3"O"^(+)]#
Now, you know that in a
In other words, you know that at equilibrium, the solution will contain
#["H"_3"O"^(+)] = "0.1 M" * 1/10 = "0.01 M" = 1 * 10^(-2)"M"#
As you know, an aqueous solution at room temperature has
#color(blue)(ul(color(black)(["H"_3"O"^(+)] * ["OH"^(-)] = 10^(-14))))#
This means that the concentration of hydroxide anions will be equal to
#["OH"^(-)] = 10^(-14)/(1 * 10^(-2)) = color(darkgreen)(ul(color(black)(1 * 10^(-12)"M")))#
Both values are rounded to one significant figure, the number of sig figs you have for the molarity of the acetic acid.