First off you're comparing an ionic bonded $\ce{HF}$ with a covalently bonded $\ce{CH4}$. HF is a stronger acid than $\ce{CH4}$ because its able to furnish out $\ce{H+}$ ions due to its ionic bonding.

So I think you're question boils down to: Why is ionic bonding in $\ce{HX}$ (X=Halogen) stronger than a covalent bond?

This is because in covalent bonding there is only a mutual agreement to share electrons whereas electrostatic attraction in ionic bonding.

First off, you're comparing an ionically bonded $\ce{HF}$ with a covalently bonded $\ce{CH4}$. HF is a stronger acid than $\ce{CH4}$ because its able to furnish out $\ce{H+}$ ions due to its ionic bonding.

So I think your question boils down to: Why is ionic bonding in $\ce{HX}$ (X=Halogen) stronger than covalent bonding?

This is because in covalent bonding there is only a mutual agreement to share electrons whereas electrostatic attraction in ionic bonding.

First off you're comparing an ionic bonded $HF$ with a covalently bonded $\ce{CH4}$. $HF$ is a stronger acid than $\ce{CH4}$ because its able to furnish out $\ce{H+}$ ions due to its ionic bonding.

So I think you're question boils down to: why is ionic bonding in $\ce{HX}$ (X=Halogen) is stronger than covalent bond.

This is because in covalent bonding there is only a mutual agreement to share electrons whereas electrostatic attraction in ionic bonding.

First off you're comparing an ionic bonded $\ce{HF}$ with a covalently bonded $\ce{CH4}$. HF is a stronger acid than $\ce{CH4}$ because its able to furnish out $\ce{H+}$ ions due to its ionic bonding.

So I think you're question boils down to: Why is ionic bonding in $\ce{HX}$ (X=Halogen) stronger than a covalent bond?

This is because in covalent bonding there is only a mutual agreement to share electrons whereas electrostatic attraction in ionic bonding.