# Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueou

Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound? Write the chemical equation for the ionization of HCOOH.
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rodclassique4r

Step 1
HCOOH is a weak electrolyte which means it will ionize/dissociate (not fully) in water in the following way:
$HCOOH\left(aq\right)⇒s{H}^{+}\left(aq\right)+HCO{O}^{-}\left(aq\right)$
That means we'd, in a given solution, have all three: and $HCO{O}^{-}$

Carl Swisher
Step 1
Formic acid is a weak electrolyte. It dissociates into $HCO{O}^{-}$ and ${H}^{+}$ ions in aqueous solution.
Step 2
Chemical equation for the ionization of HCOOH is given by,
$HCOOH\left(aq\right)⇒HCO{O}^{-}\left(aq\right)+{H}^{+}\left(aq\right)$

Don Sumner

Step 1
Different compounds show different properties in water. Electrolytes are the compounds that dissociate in aqueous solvent to give its constituent ions.
Step 2
Strong electrolytes are those that completely dissociate in its constituent ions in aqueous solution. Whereas, weak electrolytes are those that partially dissociate in its constituent ions in aqueous solution.
HCOOH constituents the cation ${H}^{+}$ and the anion $HCO{O}^{-}$.
Since HCOOH is a weak electrolyte, it will partially dissociate and will be in equilibrium with the constituent ions.
Write the equilibrium equation of the partial dissociation of HCOOH.
$HCOOH\left(aq\right)⇋{H}^{+}\left(aq\right)+HCO{O}^{-}\left(aq\right)$
Therefore, the solutes in the aqueous solution will be HCOOH, ${H}^{+}$, and $HCO{O}^{-}$ and the chemical equation for the ionization of HCOOH will be the same as its equilibrium equation.