By Joshua Suico, Updated Mar 24, 2022

Sulfuric acid (H₂SO₄) is a strong inorganic acid widely used in industry, research, and laboratories. When dissolved in water, it fully dissociates into sulfate ions (SO₄²⁻) and hydronium ions (H₃O⁺). The molarity of each ion reflects the number of moles per liter of solution and is directly linked to the initial acid concentration.

Determining Ionic Concentrations

Step 1: Write the balanced dissociation equation

H₂SO₄ + 2 H₂O → 2 H₃O⁺ + SO₄²⁻

For every mole of sulfuric acid that dissolves, 2 moles of hydronium ions and 1 mole of sulfate ions are produced.

Step 2: Calculate individual ion concentrations

With an initial concentration of 0.010 M, the molarity of each ion is obtained by multiplying the acid concentration by the stoichiometric coefficient:

• Sulfate ions: 1 × 0.010 M = 0.010 M SO₄²⁻
• Hydronium ions: 2 × 0.010 M = 0.020 M H₃O⁺

Step 3: Determine the total ionic concentration

Since one mole of H₂SO₄ yields three moles of ions, the total ionic concentration is:

3 × 0.010 M = 0.030 M of ions per liter.

TL;DR

Because sulfuric acid is a strong acid, it fully dissociates in water. For a 0.010 M solution, the concentrations are 0.010 M SO₄²⁻, 0.020 M H₃O⁺, and 0.030 M total ions.

Safety Warning

Always follow proper laboratory safety protocols when handling acids. Wear protective equipment such as lab coats, goggles, gloves, and use appropriate glassware.