Asked by Sarah
                Suppose that 85 mL of 0.4 M NaF and 50 mL of 0.4 M HCl are mixed.
What is the K for the dominant equilibrium in terms of Ka's, Kb's, Kw etc.?
Ka of HCl
1/Ka of HCl
Ka of HF
1/Ka of HF
Kb of F-
1/Kb of F-
Kb of Cl-
1/Kb of Cl-
Kw
1/Kw
There is no reaction.
            
        What is the K for the dominant equilibrium in terms of Ka's, Kb's, Kw etc.?
Ka of HCl
1/Ka of HCl
Ka of HF
1/Ka of HF
Kb of F-
1/Kb of F-
Kb of Cl-
1/Kb of Cl-
Kw
1/Kw
There is no reaction.
Answers
                    Answered by
            DrBob222
            
    millimols HCl = 0.4 x 50 = 20
millimols NaF = 85 x 9.4 = 34
.......F^- + H^+ ==> HF
I.....34.....0.......0
add.........20............
C....-20...-20.......+20
E.....14....0........20
Ka for the rxn = (HF)/(H^+)(F^-)
Doesn't that look like 1/Ka of HF to you. You could use the Henderson-Hasselbalch equation and calculate the pH of the solution.
    
millimols NaF = 85 x 9.4 = 34
.......F^- + H^+ ==> HF
I.....34.....0.......0
add.........20............
C....-20...-20.......+20
E.....14....0........20
Ka for the rxn = (HF)/(H^+)(F^-)
Doesn't that look like 1/Ka of HF to you. You could use the Henderson-Hasselbalch equation and calculate the pH of the solution.
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