Home›Calculators›Chemistry›Titration Calculator

Titration Calculator

Chemistry

Calculate titration results — equivalence point volume, unknown concentration or normality, and percent purity — for acid-base and redox titrations.

Reviewed by the thecalcu.com team · Last updated July 10, 2024

0.1
25
25
1
1
40
0.1

Primary Result

0.1
Result Type
Analyte Concentration (M)
Titrant Normality (N)
0.1
Analyte Normality (N)
0.1
Milliequivalents at Equivalence Point
2.5

This calculator computes your Primary Result, Result Type, Titrant Normality (N), Analyte Normality (N), Milliequivalents at Equivalence Point from the values you enter.

Inputs
Titration ModeTitrant Concentration (M)Titrant Volume Used (mL)Analyte Volume (mL)Titrant n-FactorAnalyte n-FactorAnalyte Molar Mass (g/mol) — for purity onlyAnalyte Mass Weighed (g) — for purity only
Outputs
Primary ResultResult TypeTitrant Normality (N)Analyte Normality (N)Milliequivalents at Equivalence Point

What is a Titration?

The Titration Calculator computes analyte concentration, equivalence point volume, or percent purity from titration data. Select the mode (find concentration, find volume, or find purity), enter titrant and analyte parameters including n-factors, and get the result with full normality and milliequivalent calculations.

Titration is the foundation of quantitative wet chemistry, from pharmaceutical QC assays to water quality analysis to food chemistry. The fundamental principle at equivalence: N₁V₁ = N₂V₂ (normality × volume of titrant = normality × volume of analyte). The n-factor (equivalents per mole) corrects for stoichiometry, H₂SO₄ has n=2 for complete neutralisation, KMnO₄ has n=5 in acidic permanganate titrations.

The Normality Calculator converts between molarity and normality using n-factors. The Molarity Calculator handles solution concentration calculations. The Neutralization Calculator covers acid-base stoichiometry for the reactions underlying acid-base titrations.

Why Use a Titration Calculator?

The N₁V₁ = N₂V₂ calculation involves converting molarity to normality via n-factors, then solving for the unknown, then optionally converting back to molarity or calculating purity. Each step requires keeping track of units (mL vs L, M vs N, meq vs mmol). This calculator handles all conversions in one step and outputs both the primary result and intermediate quantities (normalities, milliequivalents).

Who Should Use This Calculator?

Indian Class 12 students and JEE/NEET aspirants who need to solve titration problems involving molarity, normality, equivalents, and percent purity, all standard quantitative chemistry topics.

B.Sc./M.Sc. chemistry and pharmacy students at Indian universities calculating titration results for volumetric analysis practicals and assignments.

Pharmaceutical QC chemists at Indian drug manufacturers (Sun Pharma, Cipla, Dr Reddy's, Lupin) performing IP-specified titrimetric assays for API and formulation purity testing.

Water testing laboratory technicians at NABL-accredited labs computing hardness, alkalinity, COD, and chloride from EDTA, KMnO₄, and AgNO₃ titrations (per BIS IS:3025 methods).

What Insights Does the Titration Calculator Give You?

Primary Result is the main output, analyte concentration (M), required titrant volume (mL), or percent purity (%) depending on mode.

Normality of Titrant (N), titrant's equivalent concentration = molarity × n-factor.

Normality of Analyte (N), analyte's equivalent concentration, derived at equivalence.

Milliequivalents, the equivalents balance at the equivalence point (meq titrant = meq analyte).

How to use this Titration calculator

  1. Select Titration Mode: Find Unknown Concentration (most common) / Find Titrant Volume (planning) / Find Percent Purity (QC/assay).
  2. Enter Titrant Concentration (M) and Titrant Volume Used (mL) at equivalence.
  3. Enter Analyte Volume (mL), the volume of sample solution.
  4. Set n-factors: HCl n=1; H₂SO₄ n=2; NaOH n=1; Ca(OH)₂ n=2; KMnO₄ n=5; K₂Cr₂O₇ n=6; Na₂S₂O₃ n=1; EDTA n=2 (for divalent metals).
  5. For purity mode: also enter Analyte Molar Mass (g/mol) and Mass Weighed (g).
  6. Read Primary Result and check Normality and meq for verification.
Show formula & methodology ↓Show less ↑

Formula & Methodology

Titration calculation:

At equivalence point: N₁V₁ = N₂V₂  N = M × n    (Normality = Molarity × n-factor) meq = N × V(mL)   (milliequivalents)  Find unknown concentration:   N_analyte = N_titrant × V_titrant / V_analyte   M_analyte = N_analyte / n_analyte  Find titrant volume:   V_titrant = N_analyte × V_analyte / N_titrant  Find percent purity:   mol_analyte = N_analyte × V_analyte(L) / n_analyte   mass_pure = mol_analyte × MW_analyte   % purity = (mass_pure / mass_weighed) × 100  n-factor reference:   HCl: 1, H₂SO₄: 2, H₃PO₄: 3 (or 1, 2)   NaOH: 1, Ca(OH)₂: 2, Ba(OH)₂: 2   KMnO₄ (acid): 5, KMnO₄ (neutral): 3, KMnO₄ (base): 1   K₂Cr₂O₇: 6, Fe²⁺→Fe³⁺: 1, Na₂S₂O₃: 1   EDTA vs Ca²⁺ or Mg²⁺: 2

Worked example, assay of iron tablets by permanganimetry:

An iron supplement tablet weighing 0.340 g is dissolved in dilute H₂SO₄ and titrated with 0.02 N KMnO₄ (n=5, hence M = 0.004 M). At equivalence: 23.5 mL of KMnO₄ used.

Purity mode: Titrant: KMnO₄, N = 0.02 N, V = 23.5 mL Analyte: FeSO₄·7H₂O (MW = 278.01), n = 1, V = 100 mL (dissolved) Mass weighed: 0.340 g  N_analyte = 0.02 × 23.5 / 100 = 0.0047 N mol FeSO₄·7H₂O = 0.0047 × 0.1 / 1 = 0.00047 mol mass pure = 0.00047 × 278.01 = 0.1307 g % purity = 0.1307 / 0.340 × 100 = 38.4%

This is the standard IP 2022 assay for ferrous sulfate tablets, a widely prescribed haematinic in India under PMJAY (Pradhan Mantri Jan Arogya Yojana) essential medicines. Iron deficiency anaemia affects ~53% of Indian women (NFHS-5 data) and ~23% of children under 5. Government schemes (WIFS, Weekly Iron and Folic Acid Supplementation for adolescents; Anaemia Mukt Bharat for school children) distribute ferrous sulfate tablets through ASHA workers, all batches require IP assay by permanganimetry before government procurement.

Frequently Asked Questions

What is a titration in chemistry?
Titration is a quantitative analytical technique where a solution of known concentration (titrant) is added to a solution of unknown concentration (analyte) until the reaction is complete (equivalence point). The volume of titrant used and the equivalence point are measured to calculate the unknown concentration. At the equivalence point: moles of titrant × n-factor = moles of analyte × n-factor (for redox and neutralisation), or equivalently N₁V₁ = N₂V₂ (normality × volume). Titration is one of the oldest and most reliable quantitative methods, used in Indian CBSE Class 12 and B.Sc. chemistry practicals, and in Indian pharmaceutical QC under IP (Indian Pharmacopoeia) protocols.
How do I use the Titration Calculator?
Select Titration Mode: (1) Find Unknown Concentration, enter titrant concentration and n-factor, titrant volume used, analyte volume and n-factor → get analyte molarity. (2) Find Titrant Volume, enter titrant concentration, analyte volume and concentration → get volume needed for equivalence point. (3) Find Percent Purity, enter titration results plus analyte molar mass and mass weighed → get % purity. All modes show normality of both solutions and milliequivalents at equivalence. Default: 0.1 M HCl (n=1) titrating 25 mL NaOH (n=1) using 25 mL HCl at equivalence → [NaOH] = 0.1 M.
What is the equivalence principle N1V1 = N2V2?
N₁V₁ = N₂V₂ is the fundamental titration equation: normality of titrant × volume of titrant = normality of analyte × volume of analyte. At equivalence point, the milliequivalents of titrant = milliequivalents of analyte. meq = N × V(mL). N = M × n-factor (n-factor = number of equivalents per mole, see below). Example: 0.1 N H₂SO₄ (25 mL) titrating NaOH: 0.1 × 25 = N_NaOH × 25 → N_NaOH = 0.1 N. If n-factor of NaOH = 1, then [NaOH] = 0.1 M. If H₂SO₄ has n=2: N_H₂SO₄ = 0.2 × 2 = 0.2... wait, this is the key complexity the n-factor corrects for.
What is n-factor and why is it important in titrations?
The n-factor (equivalence factor) is the number of equivalents per mole of a substance, it corrects for the stoichiometry of the reaction: Acid-base: n = number of H⁺ donated (acid) or OH⁻ accepted (base). HCl: n=1; H₂SO₄: n=2; H₃PO₄: n=1, 2, or 3 depending on reaction. NaOH: n=1; Ca(OH)₂: n=2. Redox: n = number of electrons transferred. KMnO₄ in acid: n=5 (Mn⁷⁺ → Mn²⁺); K₂Cr₂O₇: n=6 (Cr⁶⁺ → Cr³⁺). Na₂S₂O₃ (thiosulfate): n=1 (vs I₂ titration). Fe²⁺: n=1 (Fe²⁺ → Fe³⁺). Precipitation: n = valency of the precipitating ion. Correct n-factor is essential for accurate normality calculation; wrong n-factor gives proportionally wrong concentration.
What are common acid-base titrations in Indian pharmacy and food analysis?
Common acid-base titrations in India: Assay of NaOH (caustic soda): 0.1 N HCl titrant, phenolphthalein indicator. N₁V₁ = N₂V₂. IP 2022 specifies this for sodium hydroxide solution assay. Assay of HCl (hydrochloric acid concentrate): 1 M NaOH titrant. Boric acid assay: H₃BO₃ complexed with mannitol, then titrated with NaOH. Aspirin (acetylsalicylic acid) potentiometric assay: NaOH standardised against potassium hydrogen phthalate (KHP). Vitamin C (ascorbic acid) assay: 2,6-dichlorophenolindophenol (DCPIP) dye titration. FSSAI (Food Safety and Standards Authority of India) requires titrimetric assay for acid content in vinegar (≥ 4% acidity as acetic acid), lemon juice, and fermented products.
What are common redox titrations in Indian analytical chemistry?
Important redox titrations: Permanganimetry (KMnO₄, n=5 in acid): Iron content in ores and supplements (FeSO₄·7H₂O iron tablets, Ferrous Ascorbate). Water COD measurement using K₂Cr₂O₇ (n=6). Iodimetry/Iodometry (Na₂S₂O₃, n=1): Vitamin C, copper sulfate assay, dissolved oxygen in water (Winkler method). Dichromatometry (K₂Cr₂O₇, n=6): Iron determination in cement (BIS IS:269), steel (SAIL QC labs). Cerimetry (Ce⁴⁺, n=1): Pharmaceutical API assays. Indian BIS standards: IS:3025 (Water and Wastewater Testing Methods) mandates permanganate value determination. Bureau of Indian Standards IS:1011 (Iron ores) uses dichromate titration for iron assay, critical for NMDC Bailadila ore grading.
What is percent purity in titration and how is it calculated?
Percent purity measures what fraction of the weighed sample is the substance of interest. % purity = (mass of pure substance / mass weighed) × 100. From titration: mass of pure substance = moles × molar mass = (N_analyte × V_analyte(L) / n-factor) × MW. If 0.50 g of impure NaOH (MW=40) requires 23.5 mL of 0.5 M HCl (n=1): moles NaOH = 0.5 × 0.0235 / 1 = 0.01175 mol. mass pure NaOH = 0.01175 × 40 = 0.470 g. % purity = 0.470/0.50 × 100 = 94.0%. Indian Pharmacopoeia (IP) specifies minimum purity requirements: IP NaOH: ≥ 97.0% NaOH. IP H₂SO₄: 95.0–97.0%. IP HCl: 35.0–38.0% w/w. NABL-accredited labs at Ranbaxy (now Sun Pharma), Dr Reddy's, and Cipla use titration-based assays for API purity certification before batch release.
What indicators are used in titrations and when?
Indicators for acid-base titrations: Phenolphthalein (pH 8.2–10.0, colourless → pink): strong acid vs strong base; strong acid vs weak base if you want alkaline endpoint. Methyl orange (pH 3.1–4.4, red → yellow): strong acid vs weak base (endpoint in acidic region). Methyl red (pH 4.4–6.2): similar to methyl orange. CBSE Class 12 standard: sodium oxalate vs KMnO₄, no indicator needed (KMnO₄ is self-indicating: decolourises until one extra drop gives persistent pink). Starch (I₃⁻ complex, deep blue): iodimetry, Na₂S₂O₃ titrations, Vitamin C. Chrome black T (EDTA titrations, complexometric): water hardness (Ca²⁺ + Mg²⁺). Potassium chromate: Mohr method for Cl⁻ (precipitation titration with AgNO₃). These are standard in NCERT practicals and IP official methods.
What is a back titration and when is it used?
Back titration adds a known excess of reagent, then titrates the unreacted excess with a second titrant. Used when: (1) The analyte is insoluble or reacts slowly. (2) No suitable indicator for direct titration. (3) End point clearer in back titration. Example: Assay of CaCO₃ purity (limestone/chalk): Add excess 0.1 N HCl to dissolve CaCO₃. CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂. Back-titrate excess HCl with 0.1 N NaOH. Moles HCl reacted with CaCO₃ = total HCl added − HCl back-titrated. CaCO₃ moles = HCl moles / 2. India's largest limestone mines (RSMML Rajasthan, Gujarat Ambuja Minerals) use back titration for CaCO₃ assay in ore grading, purity requirements differ by use (cement grade ≥ 93%, chemical/pharma grade ≥ 99%).
What is EDTA complexometric titration and how is it used in water hardness measurement?
EDTA (ethylenediaminetetraacetic acid, C₁₀H₁₆N₂O₈, MW=292) forms 1:1 complexes with nearly all metal cations. In water hardness titration: standard EDTA solution (Na₂EDTA, 0.01 M) titrates Ca²⁺ and Mg²⁺ with Eriochrome Black T (EBT) indicator at pH 10 buffer. Endpoint: wine-red → blue (EDTA displaces EBT from metal complexes). n-factor of EDTA = valency of metal being titrated (Ca²⁺: n=2; Mg²⁺: n=2; Fe³⁺: n=3). Total hardness (as CaCO₃, mg/L) = (Vol EDTA, mL × M_EDTA × 1000 × 50) / (sample vol, mL). BIS IS:10500 maximum total hardness = 300 mg/L (permissible), 200 mg/L (acceptable). Indian cities with high hardness: Delhi (220–350 mg/L), Rajasthan (400–800+ mg/L), Gujarat (300–600 mg/L). Hard water causes scaling in boilers, geysers, and pipes, a major industrial cost in India.