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Post Closed as "Needs details or clarity" by Nilay Ghosh, Jon Custer, Mithoron, Todd Minehardt, Buck Thorn♦
tried editing into something comprehensible
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Buck Thorn ♦
Buck Thorn ♦
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Well if I was wondering, if we put HF$\ce{HF}$ into a glass of water the acid will be dissolved according to this reaction: HF->F- + H+ Now

$$\ce{HF->F- + H+}$$

Now there is a proton travelling across the water.Why it is travelling is due to

All : all H20$\ce{H2O}$ molecules have equal chance of getting the proton so it travels through the liquid.Now

Now for the reaction F- + H2O ->HF + OH-

$$\ce{F- + H2O ->HF + OH-}$$

the bond strength between O and H is lower than the bond strength of F and H  (fluorine is has more electronegativity and electronegative and has a smaller atomic radius than O).According

According to Bronsted-Lowry theory for acids and bases the second reaction happens more often than the first one.But But how is this happening?The Why does the second reaction happen athappen at all.Oxygen? Oxygen is more negatively charged than fluorine so the proton would have a very small chance to reach fluorine and then the electrons would be rearranged to form the HF bond.

Well if I was wondering if we put HF into a glass of water the acid will be dissolved according to this reaction: HF->F- + H+ Now there is a proton travelling across the water.Why it is travelling is due to : all H20 molecules have equal chance of getting the proton so it travels through the liquid.Now for the reaction F- + H2O ->HF + OH- the bond strength between O and H is lower than the bond strength of F and H(fluorine is has more electronegativity and smaller atomic radius than O).According to Bronsted-Lowry theory for acids and bases the second happens more often than the first one.But how is this happening?The second reaction happen at all.Oxygen is more negatively charged than fluorine so the proton would have a very small chance to reach fluorine and then the electrons would be rearranged to form the HF bond.

I was wondering, if we put $\ce{HF}$ into a glass of water the acid will be dissolved according to this reaction:

$$\ce{HF->F- + H+}$$

Now there is a proton travelling across the water.

All $\ce{H2O}$ molecules have equal chance of getting the proton so it travels through the liquid.

Now for the reaction

$$\ce{F- + H2O ->HF + OH-}$$

the bond strength between O and H is lower than the bond strength of F and H  (fluorine is has more electronegative and has a smaller atomic radius than O).

According to Bronsted-Lowry theory for acids and bases the second reaction happens more often than the first one. But how is this happening? Why does the second reaction happen at all? Oxygen is more negatively charged than fluorine so the proton would have a very small chance to reach fluorine and then the electrons would be rearranged to form the HF bond.

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Donald Duck
Donald Duck
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Reaction of HF in water

Well if I was wondering if we put HF into a glass of water the acid will be dissolved according to this reaction: HF->F- + H+ Now there is a proton travelling across the water.Why it is travelling is due to : all H20 molecules have equal chance of getting the proton so it travels through the liquid.Now for the reaction F- + H2O ->HF + OH- the bond strength between O and H is lower than the bond strength of F and H(fluorine is has more electronegativity and smaller atomic radius than O).According to Bronsted-Lowry theory for acids and bases the second happens more often than the first one.But how is this happening?The second reaction happen at all.Oxygen is more negatively charged than fluorine so the proton would have a very small chance to reach fluorine and then the electrons would be rearranged to form the HF bond.