15 questions linked to/from Is HF the least acidic hydrogen halide?
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### Does the acid strength of hydrochloric and hydrofluoric acid correlate with the electronegativity of the halides? [duplicate]

Is this statement true or false? HCl is a stronger acid than HF because fluorine is more electronegative than chlorine. I'm thinking this is true, because since fluorine is more electronegative ...
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### Can the idea of entropy be extended to orbitals?

The forward reaction for: $\ce{HF<->H^+ +F^-}$ is entropically favourable; but energetically unfavorable: as there is too much electron density for $\ce{F^-}$ ion to cope up. That's a reason why ...
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### Hydrogen halide acidity

Why is it that $$\mathrm{p}K_\mathrm{a}(\ce{HF}) < \mathrm{p}K_\mathrm{a}(\ce{HCl}) < \mathrm{p}K_\mathrm{a}(\ce{HBr}) < \mathrm{p}K_\mathrm{a}(\ce{HI}),$$ even though the electronegativity ...
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### Solubility vs Dissociation of HF

Ok, so I understand that solubility is a measure of how well a compound is solvated by the solvent. And dissociation is a measure of how much of a compound splits into its ionized forms. Does HF have ...
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### Which of the following has a stronger hydrogen bonding: F-H- -O or F-H- -F?

I thought of two approaches to solve this question . Since the electronegativity of Oxygen is lower than Fluorine it would be a better donor than Fluorine to the electron deficient Hydrogen . Another ...
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### why HI isn't fully miscible with cold water when HF is?

HF is more soluble in water than HI , due to greater hydrogen bonding in HF , accepted but, on the other hand HF is a very weak acid so it's dissociation will be meagre when compared to HI's ...
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### How to estimate the equilibrium constant of the reaction between NaF and HCl

Since $\ce{HCl}$ is more acidic than $\ce{HF}$, the left hand side of a reaction has a stronger acid than the right hand side. Since $\ce{NaF}$ is more basic than $\ce{NaCl}$, the left hand side has ...
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### Why does HCl act as a weak base in HF solvent, even though it is a stronger acid compared to HF?

I've read that $\ce{HCl}$ acts as a weak base in $\ce{HF}$ solvent, which means $\ce{HCl}$ is supposed to lose $\ce{H+}$ ion to $\ce{HF}$. $\ce{HF}$ is a weak acid compared to $\ce{HCl}$, then shouldn'...
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### Common Ion Effect explanations

From my textbook, it is stated that: e.g. If we add a basic salt $\ce{NaF}$, it will fully dissociate to give $\ce{F-}$. Then if we add $\ce{HF}$, since it is a weak acid, the high concentration of \$\...