Calculate the concentration of all species in a 0.19 M KF solution. Please dont do it wrong...

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Chemistry

Calculate the concentration of all species in a 0.19 M KFsolution.
Please dont do it wrong its been wrong all over the internet andit makes no sense

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4.4 Ratings (636 Votes)

Â Â KF ---> K⁺ + F^- ; KF dissociates completely.

[K⁺]=[ F^-]= 0.19 M

Â Â Â Â Â Â Â Â Â Â Â Â Â Â F^-Â Â Â Â Â Â Â Â Â Â Â +Â Â Â Â Â Â Â Â Â Â Â Â H₂OÂ Â Â Â Â Â Â =Â Â Â Â Â Â Â Â Â Â Â Â HFÂ Â Â Â Â Â Â Â Â +Â Â Â Â Â Â Â Â Â Â Â Â OH^-

INitial:Â Â 0.19 MÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â

Final:Â Â Â Â 0.19-xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â x

Ka = 7.08*10^-4 ; Kb = 10^-14/7.08*10^-4 = 1.41*10^-11 = [HF][ OH^-]/[ F^-]

or, 1.41*10^-11 = x²/0.19-x = x²/0.19Â Â Â Â Â Â Â Â Â Â Â ;(as x<<0.19)

or, x = 1.64*10^-6 M

Ans: [K⁺]= 0.19 M

[F^-] = 0.19-x = 0.19 M Â Â Â ;(as x<<0.19)

[HF]= [OH^- ] =1.64*10^-6 M

[H+] = 10^Â14/1.64*10^-6 = 6.1*10^Â-9 M

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