Question #29b74
1 Answer
Explanation:
Start by looking up the acid dissociation constant for acetic acid
#K_a = 1.76 * 10^(-5)#
So, acetic acid is a weak acid that only partially ionizes in aqueous solution to produce hydronium cations and acetate anions.
#"CH"_ 3"COOH"_ ((aq)) + "H"_ 2"O"_ ((l)) rightleftharpoons "CH"_ 3"COO"_ ((aq))^(-) + "H"_ 3"O"_ ((aq))^(+)#
As you can see, every
This means that, at equlibrium, you have
#["CH"_ 3"COO"^(-)] = ["H"_ 3"O"^(+)]#
You should also know that
#color(blue)(ul(color(black)("pH" = - log(["H"_3"O"^(+)]))))#
This implies that
#["H"_3"O"^(+)] = 10^(-"pH")#
In your case, you will have
#["H"_3"O"^(+)] = 10^(-3.0) = 1.0 * 10^(-3)# #"M"#
Now, notice that the reaction consumes
This means that, at equilibrium, the concentration of the acid will be equal to
#["CH"_ 3"COOH"]_ "equil" = ["CH"_ 3"COOH"]_ 0 - ["H"_3"O"^(+)]#
Here
By definition, the acid dissociation constant will be equal to
#K_a = (["CH"_ 3"COO"^(-)] * ["H"_ 3"O"^(+)])/(["CH"_ 3"COOH"]_"equil")#
Rearrange to solve for the equilibrium concentration of the acid
#["CH"_ 3"COOH"]_ "equil" =(["CH"_ 3"COO"^(-)] * ["H"_ 3"O"^(+)])/K_a#
Plug in your values to find
#["CH"_ 3"COOH"]_ "equil" = (1.0 * 10^(-3) * 1.0 * 10^(-3))/(1.76 * 10^(-5))#
#["CH"_ 3"COOH"]_ "equil" = 5.7 * 10^(-2)# #"M"#
This means that the iniital concentration of the acid was equal to
#["CH"_3"COOH"]_0 = 5.7 * 10^(-2) color(white)(.)"M" - 1.0 * 10^(-3)color(white)(.)"M"#
#["CH"_3"COOH"]_0 = "0.056 M"#
Finally, to find the volume of glacial acetic acid needed to make this solution, use the fact that the dilution factor is equal to
#"DF" = (17.4 color(red)(cancel(color(black)("mL"))))/(0.056color(red)(cancel(color(black)("mL")))) = color(blue)(310.7)#
This means that you have
#"DF" = V_"diluted"/V_"stock" implies V_"stock" = V_"diluted"/"DF"#
which, in your case, is equal to
#V_"stock" = "1.0 L"/color(blue)(310.7) = "0.003226 L"#
Expressed in milliliters and rounded to two sig figs, the answer will be
#color(darkgreen)(ul(color(black)(V_"stock" = "3.2 mL")))#