Determine the [H3O^+] of a 0.240 M solution of formic acid.

HCOOH ==> H^+ + HCOO^-

Ka = (H^+)(HCOO^-)/(HCOOH)
Set up an ICE chart, substitute into the Ka expression and solve for H^+.

To determine the [H3O^+] concentration of a solution of formic acid, we need to consider the ionization of formic acid, which is a weak acid. The chemical equation for the ionization of formic acid (HCOOH) is as follows:

HCOOH (aq) ⇌ H^+ (aq) + HCOO^-

The equilibrium constant expression for this reaction is given by:

Ka = [H^+] [HCOO^-] / [HCOOH]

The concentration of formic acid is given as 0.240 M.

Since formic acid is a weak acid, we can assume that its ionization is only partially complete. Thus, the concentration of H^+ is equal to the concentration of formic acid that has ionized.

Therefore, we can assume that [H^+] = 0.240 M.

Thus, the [H3O^+] concentration in the 0.240 M solution of formic acid is 0.240 M.

To determine the concentration of the hydronium ion, [H3O+], in a solution of formic acid, we will first need to understand the acid dissociation reaction of formic acid.

The formula for formic acid is HCOOH, and it can dissociate in water as follows:

HCOOH + H2O ⇌ H3O+ + HCOO-

From this reaction, we can see that one molecule of formic acid yields one hydronium ion. Therefore, the concentration of the hydronium ion, [H3O+], will be equal to the concentration of formic acid, [HCOOH], in the solution.

In this case, the concentration of formic acid is given as 0.240 M. Hence, the [H3O+] of the 0.240 M solution of formic acid is also 0.240 M.