Question

Formic acid, from the Latin formica, is the acid present in ants sting. What is the

Answer 1

For the reaction of deprotonation of formic acid, the concentration of HCOO⁻ at equilibrium is 0.0151 M if the initial concentration of formic acid is 1.35 M.  

The reaction of deprotonation of formic acid is the following:

CHOOH + H₂O ⇄ HCOO⁻ + H₃O⁺

At the equilibrium we have:

CHOOH + H₂O ⇄ HCOO⁻ + H₃O⁺    (1)

1.35 - x                         x           x

The acid equilibrium constant for this reaction is:

$K_{a} = \frac{[HCOO^{-}][H_{3}O^{+}]}{[CHOOH]} = 1.7 \cdot 10^{-4}$  (2)

Entering the values of [CHOOH] = 1.35-x, [HCOO⁻] = [H₃O⁺] = x, into equation (2) we have:

$1.7 \cdot 10^{-4} = \frac{[HCOO^{-}][H_{3}O^{+}]}{[CHOOH]} = \frac{x^{2}}{(1.35 - x)}$  

$1.7 \cdot 10^{-4}(1.35 - x) - x^{2} = 0$

After solving the above quadratic equation and taking the positive value for x (concentrations cannot be negative), we have:

$x = [HCOO^{-}] = [H_{3}O^{+}] = 0.0151 M$

Therefore, the concentration of HCOO⁻ at equilibrium is 0.0151 M.

Learn more about the equilibrium constant here:

• brainly.com/question/7145687?referrer=searchResults

• brainly.com/question/9173805?referrer=searchResults

I hope it helps you!