Titration Calculator

Solve titration problems by calculating unknown concentrations, required volumes, or verifying moles at equivalence point. Enter stoichiometric coefficients from your balanced equation and known values.

Titration Formula: M₁V₁/n₁ = M₂V₂/n₂ Where: • M₁ = Molarity of analyte (unknown concentration) • V₁ = Volume of analyte • n₁ = Stoichiometric coefficient of analyte • M₂ = Molarity of titrant (standard solution) • V₂ = Volume of titrant used • n₂ = Stoichiometric coefficient of titrant Solving for Different Variables: 1. Unknown Concentration: M₁ = (M₂ × V₂ × n₁)/(V₁ × n₂) 2. Volume Required: V₁ = (M₂ × V₂ × n₁)/(M₁ × n₂) V₂ = (M₁ × V₁ × n₂)/(M₂ × n₁) 3. Moles at Equivalence: Moles = M × V (in liters) At equivalence: moles₁/n₁ = moles₂/n₂ 4. Molarity Definition: M = moles/volume(L) M = (mass/molar mass)/volume(L) Common Reactions: • HCl + NaOH → NaCl + H₂O (1:1) • H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O (1:2) • 2HCl + Ba(OH)₂ → BaCl₂ + 2H₂O (2:1) • CH₃COOH + NaOH → CH₃COONa + H₂O (1:1)
Example 1: Find Unknown HCl Concentration (1:1 ratio) Given: • 25.0 mL HCl (unknown concentration) • 30.5 mL of 0.100 M NaOH used • Reaction: HCl + NaOH → NaCl + H₂O (n₁=1, n₂=1) M₁ = (0.100 × 30.5 × 1)/(25.0 × 1) = 0.122 M HCl Moles HCl = 0.122 × 0.025 = 0.00305 mol Moles NaOH = 0.100 × 0.0305 = 0.00305 mol ✓ Example 2: Find Volume of H₂SO₄ Needed (1:2 ratio) Given: • 0.150 M H₂SO₄ (unknown volume) • 40.0 mL of 0.200 M NaOH • Reaction: H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O (n₁=1, n₂=2) V₁ = (0.200 × 40.0 × 1)/(0.150 × 2) = 26.7 mL H₂SO₄ Moles H₂SO₄ = 0.150 × 0.0267 = 0.00400 mol Moles NaOH = 0.200 × 0.040 = 0.00800 mol Check: 0.00400/1 = 0.00800/2 = 0.00400 ✓ Example 3: Standardize NaOH with KHP (1:1) Given: • 0.500 g KHP (204.22 g/mol) dissolved in 25.0 mL • 23.4 mL NaOH used • Reaction: KHP + NaOH → KNaP + H₂O (n₁=1, n₂=1) Moles KHP = 0.500/204.22 = 0.002448 mol M₁ (KHP) = 0.002448/0.025 = 0.0979 M M₂ (NaOH) = (0.0979 × 25.0 × 1)/(23.4 × 1) = 0.1046 M Example 4: Polyprotic Acid H₂SO₄ (1:2) Given: • 20.0 mL of 0.250 M H₂SO₄ • Find volume of 0.500 M NaOH needed V₂ = (0.250 × 20.0 × 2)/(0.500 × 1) = 20.0 mL NaOH Note: H₂SO₄ is diprotic, so n₁=1 but n₂=2 for complete neutralization

What is titration?

Titration is a laboratory technique to determine the concentration of an unknown solution by reacting it with a solution of known concentration (standard solution) until the reaction is complete, indicated by a color change or pH meter.

How does the titration formula work?

The formula M₁V₁/n₁ = M₂V₂/n₂ is based on the fact that moles of acid = moles of base at equivalence point. M is molarity, V is volume, and n is the stoichiometric coefficient from the balanced equation.

What is molarity?

Molarity (M) is moles of solute per liter of solution: M = mol/L. It's the standard concentration unit in chemistry. Example: 0.1 M HCl means 0.1 moles of HCl per liter of solution.

Why do I need stoichiometric ratios?

Different acids and bases react in different mole ratios. HCl + NaOH is 1:1, but H₂SO₄ + 2NaOH is 1:2. The stoichiometric coefficients (n₁, n₂) from the balanced equation ensure accurate concentration calculations.

What is the equivalence point?

The equivalence point is when moles of acid equal moles of base (adjusted for stoichiometry). It's detected by indicators (color change) or pH meters. For strong acid-strong base, equivalence point pH = 7.

Can I solve for different variables?

Yes! This calculator solves for unknown concentration (most common), volume needed, or moles. Just select what you want to find and enter the known values from your titration data.

What are common acid-base pairs?

Strong acid-strong base: HCl-NaOH (1:1), H₂SO₄-NaOH (1:2). Weak acid-strong base: CH₃COOH-NaOH (1:1). Strong acid-weak base: HCl-NH₃ (1:1). Always write balanced equations for stoichiometry.

How do I convert mL to L?

Divide by 1000: L = mL ÷ 1000. Example: 25 mL = 0.025 L. Molarity uses liters, but titration volumes are often measured in mL, so conversion is essential for calculations.