Titration Calculator

Calculate concentration, volume, pH at equivalence point, and generate titration curves for acid-base titrations.

Basic Titration Calculator (M₁V₁ = M₂V₂)

Calculate unknown concentration or volume using the titration equation.

Analyte (Solution Being Titrated)
Titrant (Solution in Burette)
For HCl + NaOH → NaCl + H₂O, ratio is 1:1. For H₂SO₄ + 2NaOH, ratio is 1:2
Example Problems:
⭐ Basic (1:1 Stoichiometry)
Find M₁: 25mL HCl + 16.7mL 0.150M NaOH Find V₂: 25mL 0.100M HCl + ? 0.150M NaOH Find M₂: 20mL 0.100M acid + 15.5mL NaOH Find V₁: ? 0.250M HNO₃ + 30mL 0.100M KOH Find M₁: 50mL CH₃COOH + 25mL 0.200M NaOH
⭐⭐ Polyprotic Acids (1:2 Stoichiometry)
Find M₁: H₂SO₄ + 2NaOH (18.5mL 0.200M) Find V₂: 15mL 0.150M H₂SO₄ + 2NaOH Find M₁: H₂C₂O₄ + 2KOH (45mL 0.100M)
⭐⭐⭐ Triprotic Acids (1:3 Stoichiometry)
Find V₂: 10mL 0.100M H₃PO₄ + 3NaOH Find M₁: H₃PO₄ + 3KOH (35mL 0.120M)
🧪 Reverse Titrations (Base as Analyte)
Find M₁: 30mL NaOH + 22.5mL 0.200M HCl Find V₂: 40mL 0.080M Ba(OH)₂ + HCl (2:1)
pH at Equivalence Point

Calculate the pH at the equivalence point for strong or weak acid/base titrations.

Acid
Base
Example Problems:
⭐ Strong Acid + Strong Base (pH = 7.0)
HCl + NaOH (0.1M, 25mL each) HNO₃ + KOH (0.2M/0.15M) HCl + NaOH (dilute 0.05M)
⭐⭐ Weak Acid + Strong Base (pH > 7)
CH₃COOH + NaOH (Ka=1.8×10⁻⁵) HNO₂ + KOH (Ka=6.3×10⁻⁵) HF + NaOH (Ka=6.5×10⁻⁵) HCOOH + KOH (Ka=1.3×10⁻⁵) HCN + NaOH (Ka=4.9×10⁻¹⁰)
⭐⭐ Strong Acid + Weak Base (pH < 7)
HCl + NH₃ (Kb=1.8×10⁻⁵) HNO₃ + NH₃ (Kb=1.8×10⁻⁵) H₂SO₄ + CH₃NH₂ (Kb=4.4×10⁻⁴)
⭐⭐⭐ Various Weak Acids
HClO₂ + NaOH (Ka=1.8×10⁻⁴) HF₂⁻ + KOH (Ka=6.6×10⁻⁴)
Titration Curve Generator

Generate a pH vs volume titration curve.

Example Curves:
⭐ Strong Acid + Strong Base (Sharp Curve)
HCl + NaOH (0.1M standard) HNO₃ + KOH (2:1 conc) HCl + NaOH (dilute)
⭐⭐ Weak Acid + Strong Base (Buffer Region)
CH₃COOH + NaOH (Ka=1.8×10⁻⁵) CH₃COOH dilute (0.05M) HNO₂ + KOH (Ka=6.3×10⁻⁵) HF + NaOH (Ka=6.5×10⁻⁵) HCN + NaOH (very weak)
⭐⭐⭐ Compare Strong vs Weak
Strong (HCl) Weak (CH₃COOH) Medium weak (HClO₂)
Results


Enter data and click Calculate to see results

Understanding Titrations
Titration Basics

A titration is a technique to determine the concentration of an unknown solution by reacting it with a solution of known concentration.

Key Terms
  • Analyte: The solution being analyzed (in flask)
  • Titrant: The solution of known concentration (in burette)
  • Equivalence Point: When moles of acid = moles of base
  • Endpoint: When indicator changes color
Titration Equation

M₁V₁/n₁ = M₂V₂/n₂

Where M = molarity, V = volume, n = stoichiometric coefficient

pH at Equivalence Point
  • Strong + Strong: pH = 7.0
  • Weak Acid + Strong Base: pH > 7 (basic)
  • Strong Acid + Weak Base: pH < 7 (acidic)
  • Weak + Weak: Depends on Ka and Kb

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