HCHO2 = 1.77 * 10^-4
If the concentration of formic acid (HCHO2) is 1.24 M, what is the concentration of H30+ in the solution?
First write your equation with water included.
HCHO2 + H20 --> H3O+(aq) + HCO2-
Then construct an ICE (initial, change, final) table.
To determine the concentration of H30+ in the solution, we need to consider the dissociation of formic acid (HCHO2) and use an equilibrium expression.
The dissociation of formic acid can be represented as follows:
HCHO2 ⇌ H+ + CHO2-
The equilibrium expression for this reaction can be written as:
K = [H+][CHO2-] / [HCHO2]
Given that the equilibrium constant (K) for this reaction is 1.77 * 10^-4, we can express it as:
1.77 * 10^-4 = [H+][CHO2-] / [HCHO2]
Since the concentration of formic acid ([HCHO2]) is 1.24 M, we can substitute this value into the equation:
1.77 * 10^-4 = [H+][CHO2-] / (1.24 M)
To solve for [H+], we rearrange the equation:
[H+] = (1.77 * 10^-4) * (1.24 M) / [CHO2-]
The concentration of CHO2- can be assumed to be negligible compared to the initial concentration of formic acid, so we can ignore it for simplicity.
Therefore, the concentration of H30+ in the solution, [H+], is approximately equal to:
[H+] = (1.77 * 10^-4) * (1.24 M)
[H+] = 2.192 * 10^-4 M
Hence, the concentration of H30+ in the solution is approximately 2.192 * 10^-4 M.