If you want to prepare a solution that has #"pH" = 8.51# at #25^@ "C"#, what initial concentration of #"NaF"# would you need to achieve?
2 Answers
Explanation:
You need to look up
From the ICE table you get this expression:
I am also getting approximately
As I mentioned earlier, you were given the pH which allows you to find the equilibrium concentration of
#"F"^(-)(aq) + "H"_2"O"(l) rightleftharpoons "HF"(aq) + "OH"^(-)(aq)#
#"I"" "c" M"" "" "" "-" "" "" ""0 M"" "" ""0 M"#
#"C"" "-x " ""M"" "-" "" "+x " M"" "+x" M"#
#"E"" "(c - x) "M"" "-" "" "" "x" M"" "" "x" M"#
where we let
You should have the
Therefore,
#K_b = (["HF"]["OH"^(-)])/(["F"^(-)]) = x^2/(c - x)#
Since we were given that
#["OH"^(-)]# at equilibrium is#10^(-"pOH") = 3.236xx10^(-6)# #"M" = x# .
This means we already solved for
#K_b = (3.236xx10^(-6) "M")^2/(c - 3.236xx10^(-6) "M") = 1.479xx10^(-11)#
By the small
As a result, our evaluation simplifies to (where
#(1.479xx10^(-11) "M")c = (3.326xx10^(-6) "M")^2#
#=> color(blue)(c = ["F"^(-)] = ["NaF"] = "0.708 M")#