Respuesta :
The fluoride ion concentration is 1.4 x [tex]10^-^3[/tex], and the solution's pH is 1.
The main species in solution are [tex]H^+[/tex], [tex]Cl^-[/tex], HF, and the solvent [tex]H_2O[/tex] since HCl is a strong acid and HF is a weak acid. The question requests the fluoride ion concentration [[tex]F^-[/tex]], which are created when HF is ionized. Consequently, the crucial equation is:
[tex]HF (aq) \leftrightarrow H^+ (aq) + F^- (aq)[/tex]
Equilibrium 0.20 – x mol 0.10 + x mol 0 + x mol
Equilibrium constant = 6.8 x [tex]10^-^4[/tex]
[tex]Ka = \frac{[H^+][F^-]}{[HF]}[/tex]
6.8 x [tex]10^-^4[/tex] = [0.10] [x] / [0.20]
x = (0.20 / 0.10) x 6.8 x [tex]10^-^4[/tex]
x = 1.4 x [tex]10^-^3[/tex]
Fluoride ion concentration, [[tex]F^-[/tex]] = 1.4 x [tex]10^-^3[/tex]
[[tex]H^+[/tex]] = (0.10 +x) = 0.10M
Thus, pH = 1.00 since it is entirely from HCl and HF has negligible contribution.
Result:
The fluoride ion concentration is 1.4 x [tex]10^-^3[/tex] and the pH of the solution is 1.00.
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