Sulfuric Acid - A Substance Requiring Special Handling!

Sulfuric acid is a chemical compound known for its corrosive and toxic properties. Despite its hazards, it plays a vital role across various industries.

In fact, it is used to manufacture products you interact with daily. Sulfuric acid serves as a raw material in detergents, batteries, and the removal of impurities from petroleum during the refining process.

In this article, we explore sulfuric acid, its primary applications, and the essential emergency response protocols for accidental exposure.

What is Sulfuric Acid?

Sulfuric acid or H2SO4 is a highly corrosive substance that inflicts severe damage on the skin, eyes, teeth, and lungs. Long-term exposure or high doses can be fatal. The severity of health risks largely depends on the dosage, exposure duration, and specific workplace hazards involved.

Pure sulfuric acid exhibits extreme corrosiveness toward other materials. Acting as a strong acid, a powerful dehydrating agent, and an oxidant, it reacts aggressively upon contact.

Furthermore, sulfuric acid is hygroscopic, readily absorbing moisture from the surrounding air. Mixing sulfuric acid with water generates an intense exothermic reaction (releasing significant heat). Direct contact with pure sulfuric acid causes chemical burns alongside severe thermal burns due to immediate tissue dehydration.

An Essential Commodity

Sulfuric acid stands as a critical commodity chemical, so much so that a nation's consumption of it often serves as a key indicator of its industrial strength. It is synthesized on an industrial scale using various methods, including the contact process, wet sulfuric acid process, lead chamber process, and other specialized techniques.

As a cornerstone of the chemical industry, one of its most widespread applications is in the production of agricultural fertilizers.

How is Sulfuric Acid Produced?

The production of sulfuric acid typically involves three main stages:

1. Formation of sulfur dioxide gas SO2

2. Catalytic oxidation of sulfur dioxide to sulfur trioxide SO3.

3. Double-contact absorption of sulfur trioxide into sulfuric acid H2SO4

Physical and Chemical Properties of Sulfuric Acid

1. Physical Properties

• Molecular Weight / Molar Mass: 98,079 g/mol

• Density: 1,84 g/cm^3

• Boiling Point: 337 degree Celsius

• Melting Point: 10 degree Celsius

• Vapor Pressure:  0,001 mmHg pada 25 degree Celsius

2. Chemical Properties

Sulfuric acid reacts readily with most bases to form sulfates. For example, electroplating solutions often prepare copper(II) sulfate by reacting copper(II) oxide with sulfuric acid:

It can displace weaker acids from their salts. For instance, reacting sulfuric acid with sodium acetate yields acetic acid and sodium bisulfate:

Dilute sulfuric acid attacks reactive metals, such as iron, aluminum, zinc, manganese, magnesium, and nickel, via single-displacement reactions, yielding hydrogen gas and metal salts:

Hazards of Sulfuric Acid

Sulfuric acid poses severe hazards to human health, the environment, and industrial facilities:

1. Health Side Effect

The corrosive nature of sulfuric acid causes severe tissue burns. Inhaling sulfuric acid vapors leads to severe respiratory tract irritation.

Prolonged or chronic exposure can cause persistent respiratory complications. Additionally, when reacting with certain substances, it can release toxic gases such as sulfur dioxide.

2. Environmental Impact

Sulfuric acid is a major contributor to acid rain.

When atmospheric wind currents transport sulfuric acid particles, they mix with moisture and fall back to Earth as precipitation.

Acid rain severely damages vegetation, forests, and freshwater ecosystems, while accelerating the degradation of buildings and metallic structures.

3. Industrial Hazards

Because industries such as chemical manufacturing, petrochemicals, and processing plants rely heavily on sulfuric acid, strict Occupational Health and Safety (OHS/K3) standards are mandatory. Mishandling can lead to catastrophic industrial accidents, while unmanaged sulfuric acid waste poses grave risks of severe environmental contamination.

Applications of Sulfuric Acid

Sulfuric acid is a key component in the production and processing of:

• Detergents and cleaning agents

• Nitric acid synthesis

• Lead-acid batteries

• Removal of impurities during petroleum refining

• Explosive materials (e.g., nitroglycerin synthesis)

• Synthetic chemical fertilizers

• Rayon manufacturing (combined with copper tetrammine)

• Industrial adhesives and glues

• Laboratory chemical reagents

• Water treatment chemical processes

Laboratory Handling and First Aid Protocols if in Contact with Sulfuric Acid

In the event of accidental exposure, immediate emergency protocols must be followed before seeking medical attention:

a. Skin Contact

Flush the affected area immediately with large amounts of running water. Remove contaminated clothing promptly while rinsing. Rapid response is critical to limit severe chemical and thermal tissue damage.

b. Severe Burns

Provide first aid continuously while waiting for emergency medical services. Do not apply oils, ointments, or salves to acid burns.

c. Ingestion: Do not induce vomiting

Inducing vomiting causes re-exposure of the esophagus, throat, and mouth to the corrosive acid. Instead, administer water in large quantities to dilute the acid in the stomach. Alternatively, milk mixed with egg whites can be administered if available.

d. Storage & Equipment

Store sulfuric acid in designated, corrosion-resistant containers isolated from incompatible chemicals. Use acid-resistant glassware or specialized plastics when handling it. Avoid metal equipment, as sulfuric acid rapidly corrodes reactive metals.

Sulfuric Acid Should be Handled with Care

Sulfuric acid can be beneficial, but needs to be handled with extra care because it is hazardous properties.

In AMI Scientific, there is sulfuric acid as a reagent and for laboratory. Click here for further information!