Calculate the pH of mixtures containing strong acids (HCl, H₂SO₄, HNO₃) and strong bases (NaOH, KOH, Ba(OH)₂). Enter concentrations and volumes for each component, and see the resulting pH after neutralization.
Add strong acids, bases, and/or salts with their concentrations and volumes to calculate the pH after mixing.
Strong electrolytes are substances that completely dissociate into ions when dissolved in water. This includes strong acids (like HCl, H₂SO₄, HNO₃), strong bases (like NaOH, KOH, Ba(OH)₂), and most ionic salts.
When you mix strong acids and bases, they undergo neutralization: H⁺ + OH⁻ → H₂O. The pH of the final mixture depends on which species is in excess after neutralization.
Step 1: Calculate moles of each acid and base from concentration (mol/L) and volume (L).
Step 2: Neutralization occurs until one species is depleted. Find the excess.
Step 3: Calculate the concentration of excess H⁺ or OH⁻ in the total volume.
Step 4: Calculate pH from [H⁺], or use pH = 14 − pOH if base is in excess.
Mix 50 mL of 0.1 M HCl with 30 mL of 0.1 M NaOH
The mixture is acidic because there's excess HCl after neutralization.
Weak acids (acetic acid) and weak bases (ammonia) require equilibrium calculations with Ka or Kb values.
For buffer solutions (weak acid + conjugate base), use the Henderson-Hasselbalch equation tool instead.
Assumes dilute solutions with complete dissociation. Real solutions may show deviations at high concentrations.
Uses Kw = 10⁻¹⁴ which is valid at 25°C. At different temperatures, Kw and neutral pH change.
Educational Use Only
This tool provides simplified calculations for learning and homework-style problems about strong electrolyte mixtures. It assumes complete dissociation and ideal behavior. Do NOT use for industrial waste neutralization, pharmaceutical formulation, or any application requiring precise pH control. Real laboratory work requires proper training, safety equipment, and professional guidance.
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