Question

$KF$is a strong electrolyte, and $HF$is a weak electrolyte. How is the solution of $KF$ different from that of $HF$?

Short answer

$KF$is strong electrolyte and it separates into ions when dissolved in water.

$HF$ is a weak electrolyte and that are partially ionized into water.

Step-by-step solution

Introduction.

Electrolytes are substances with whom the aqueous solution conduct electric current. There are primarily two kinds:

1. Strong electrolytes.
2. Weak electrolytes

Strong electrolytes have the following characteristics: They are made up of ionic compounds. When mixed with water, they totally detached into their ions. They conduct electricity in solution attributed to the prevalence of ions, but not in solid form because neutral molecules do not conduct electricity.

Weak electrolytes are partially ionized substances in water. In general, strong electrolytes seem to be acidic and base, whereas weak electrolytes are acidic and base.

Given Information.

$KF$is a strong electrolyte and $HF$is a weak electrolyte.

To know the difference between that two electrolyte.

Explanation.

$KF$is an example of a strong electrolyte that totally differentiates into its ions because once dissolved in water, so even though $HF$is an example of a weak electrolyte which temporarily ionizes when mixed with water. $K^{+}$and $F^{-}$are the only ions are present in $KF$, because although $HF$substance is dissolved only $H^{+}$and $F^{-}$ions, as well as undissociated $HF$molecules.

$\mathrm{KF}\left(s\right)\underset{\text{Dissociation}}{\stackrel{\mathrm{H},\mathrm{O}}{⟶}}{\mathrm{K}}^{+}\left(aq\right)+{\mathrm{F}}^{-}\left(aq\right)$