Ionic EquilibriumHard
Question
Which is/are correct statements :
(i) In any strong acid’s solution, the concentration of [OH-] will be zero.
(ii) If DGo of a reaction is positive, then the reaction will not proceed at all, in the forward direction for any concentrations of reactants and products.
(iii) Titration curves are drawn for (about the figure shown)
(a) 1M HCl (50 mL) with 1 M NaOH and
(b) 0.01 M HCl (50 mL) with 0.01 M NaOH on the same graph paper they look like:
(i) In any strong acid’s solution, the concentration of [OH-] will be zero.
(ii) If DGo of a reaction is positive, then the reaction will not proceed at all, in the forward direction for any concentrations of reactants and products.
(iii) Titration curves are drawn for (about the figure shown)
(a) 1M HCl (50 mL) with 1 M NaOH and
(b) 0.01 M HCl (50 mL) with 0.01 M NaOH on the same graph paper they look like:
Options
A.i & ii
B.iii only
C.ii only
D.i & iii
Solution
(i) False, [OH-] = 
at 25oC
=
at any other temperature
(ii) False, ᐃGo = 0 = - RT ln Keq
so, Keq = 1
Hence reaction will proceed significantly in the forward direction.
at 25oC =
at any other temperature(ii) False, ᐃGo = 0 = - RT ln Keq
so, Keq = 1
Hence reaction will proceed significantly in the forward direction.
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