Formic Acid and Sodium Hydroxide

HCOOH + NaOH → HCOONa + H₂O

Overview

Formic acid, the simplest carboxylic acid, reacts with sodium hydroxide to form sodium formate and water. Formic acid (Ka = 1.8 × 10⁻⁴) is about 10 times stronger than acetic acid. It was originally obtained by distillation from ants (Latin: formica).

Participants

Role	Substance	Coefficient	State
Reactant	Formic Acid CH₂O₂	1	(aq)
Reactant	Sodium Hydroxide NaOH	1	(aq)
Product	Water H₂O	1	(l)

Everyday Example

Formic acid causes the burning sensation of ant bites and bee stings, which can be neutralized by applying a basic paste like baking soda.

Industrial Importance

Sodium formate is used as a de-icing agent for airport runways, as a leather tanning agent, and as a reducing agent in organic synthesis.

Properties

Type: Acid-Base
Reversible: No
Energy: Exothermic
ΔH: -56.5 kJ/mol

Related Reactions

Acetic Acid and Sodium Acetate Buffer System Acetic Acid and Sodium Hydroxide Neutralization Acetic Acid Dissociation in Water Aluminum Chloride and Chloride Ion (Lewis Acid-Base) Aluminum Hydroxide as Amphoteric Acid with NaOH Aluminum Hydroxide as Amphoteric Base with HCl Ammonia and Ammonium Chloride Buffer System Ammonia and Hydrochloric Acid Ascorbic Acid and Sodium Hydroxide Barium Hydroxide and Ammonium Thiocyanate (Endothermic)

Frequently Asked Questions

What is the equation for Formic Acid and Sodium Hydroxide?

The balanced equation is: HCOOH + NaOH → HCOONa + H₂O.

What type of reaction is Formic Acid and Sodium Hydroxide?

Formic Acid and Sodium Hydroxide is a acid-base reaction.

Is Formic Acid and Sodium Hydroxide exothermic or endothermic?

Formic Acid and Sodium Hydroxide is exothermic (releases energy). The enthalpy change (ΔH) is -56.5 kJ/mol.