Titration Calculator
Calculate unknown acid or base concentration, burette volume, or titrated amount from routine acid-base titration data. This page is built for single-step titration math, classroom chemistry, and lab notebooks where stoichiometric coefficients matter.
Edited by Gail Joyce
Gail Joyce edits core chemistry calculator pages for formula clarity, unit consistency, and practical classroom and lab-use readability.
This calculator page is maintained by the Chemistry Calculators editorial team. The titration formulas, stoichiometric relationships, worked examples, and terminology on this page are reviewed against standard analytical chemistry methods and commonly used general chemistry reference material before major updates.
When to Use This Titration Calculator
Use this page when you are solving a standard acid-base titration and already know enough measured values to solve for one unknown. It is best for classroom neutralization problems, burette calculations, and lab reports where you need molarity or volume from a balanced reaction.
This page does not replace a full titration curve tool, buffer pH workflow, or back-titration planner. Use it when the job is straightforward titration stoichiometry with one unknown value.
Homework verification
Check neutralization math, coefficient handling, and unit conversions before you write up the answer.
Routine lab titrations
Use it after you record burette readings and standard solution concentrations for a single endpoint calculation.
Stoichiometric checks
Use it when the balanced equation is not 1:1 and you need the coefficient ratio included correctly.
Titration Calculator
Enter known values to calculate unknown molarity, volume, or titrated amount. For non-1:1 stoichiometry, adjust coefficients.
Scope: this calculator is for single-step acid-base titration math after you know the balanced reaction. It is not a titration curve simulator or indicator-selection tool.
Table of Contents
Quickly navigate to different sections of this guide. Click any item below to jump to that section.
Understanding Titration Math
In a standard acid-base titration, a solution of known concentration reacts with an analyte until the balanced reaction reaches its equivalence relationship. That lets you relate measured volume and concentration data to an unknown value without solving the chemistry from scratch each time.
For 1:1 neutralization reactions such as HCl with NaOH, the relationship is often written as M₁V₁ = M₂V₂. When the balanced equation uses different coefficients, the full stoichiometric form is n₁M₁V₁ = n₂M₂V₂. This page focuses on that calculation step, not on plotting a full titration curve or choosing an indicator.
How to Use the Titration Calculator
Work in the same order you would in a lab book: identify the missing value, confirm the balanced reaction, and then enter the measured titration data with matching volume units.
Choose the unknown you need
Decide whether you are solving for the concentration or volume of the acid or base so you know which field should remain blank.
Enter the measured titration values
Fill in the known molarity and volume fields from your burette reading, flask volume, or prepared standard solution.
Set the reaction coefficients correctly
Keep both coefficients as 1 for reactions like HCl + NaOH. Change them when the balanced equation is not 1:1, such as H₂SO₄ with NaOH.
Check units, then calculate
Use matching volume units on both sides before calculating. Then review the result and the worked steps to confirm the answer belongs to the correct solution.
Formulas and Equations
Titration calculations use fundamental stoichiometric relationships. Here's how each formula works:
Core Titration Formulas
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For 1:1 Stoichiometry: M₁V₁ = M₂V₂
At the equivalence point, moles of acid equal moles of base. This gives M₁V₁ = M₂V₂, where M is molarity and V is volume.
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For Non-1:1 Stoichiometry: n₁M₁V₁ = n₂M₂V₂
When stoichiometric coefficients differ, multiply by the coefficients. For example, H₂SO₄ + 2NaOH requires 2M₁V₁ = M₂V₂.
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Calculate Unknown Molarity: M₂ = (n₁M₁V₁)/(n₂V₂)
Rearrange the equation to find the unknown molarity when volume is known.
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Calculate Unknown Volume: V₂ = (n₁M₁V₁)/(n₂M₂)
Rearrange the equation to find the unknown volume when molarity is known.
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Moles from Titration: moles = MV (in liters)
Calculate moles from molarity and volume. Remember to convert mL to L: moles = M × (V/1000) for volumes in mL.
Worked Examples
Let's work through detailed examples showing how to calculate titration parameters step by step. These examples cover common scenarios you'll encounter in analytical chemistry.
Example 1: Calculate Unknown Molarity (1:1 Stoichiometry)
Scenario: 25.0 mL of 0.100 M NaOH is required to titrate 30.0 mL of HCl solution. What is the molarity of the HCl solution?
Solution:
Step 1: Identify known values
M₁ = 0.100 M (NaOH), V₁ = 25.0 mL, V₂ = 30.0 mL (HCl)
Step 2: Apply the titration equation
M₁V₁ = M₂V₂ (1:1 stoichiometry)
M₂ = M₁V₁/V₂ = (0.100 M × 25.0 mL) / 30.0 mL = 0.0833 M
Answer: HCl molarity = 0.0833 M
Example 2: Calculate Unknown Volume (1:1 Stoichiometry)
Scenario: How many mL of 0.150 M HCl are needed to titrate 20.0 mL of 0.200 M NaOH?
Solution:
Step 1: Identify known values
M₁ = 0.150 M (HCl), M₂ = 0.200 M (NaOH), V₂ = 20.0 mL
Step 2: Apply the titration equation
M₁V₁ = M₂V₂
V₁ = M₂V₂/M₁ = (0.200 M × 20.0 mL) / 0.150 M = 26.7 mL
Answer: Volume of HCl = 26.7 mL
Example 3: Non-1:1 Stoichiometry
Scenario: 40.0 mL of 0.100 M H₂SO₄ requires 35.0 mL of NaOH solution for complete neutralization. What is the molarity of the NaOH solution? (H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O)
Solution:
Step 1: Identify stoichiometric coefficients
n₁ = 1 (H₂SO₄), n₂ = 2 (NaOH)
Step 2: Apply the modified titration equation
n₁M₁V₁ = n₂M₂V₂
2M₂V₂ = M₁V₁
M₂ = M₁V₁/(2V₂) = (0.100 M × 40.0 mL) / (2 × 35.0 mL) = 0.0571 M
Answer: NaOH molarity = 0.0571 M
Common Titration Mistakes to Avoid
Using the final burette reading instead of delivered volume
Always subtract the initial burette reading from the final reading unless the burette started at exactly 0.00 mL.
Leaving stoichiometric coefficients at 1 for every reaction
If the balanced equation is not 1:1, update the coefficient fields before you calculate.
Mixing liters and milliliters without checking
Use matching volume units on both sides of the calculation or convert first so the ratio stays valid.
Frequently Asked Questions
These are the questions users most often need when checking titration math, reaction ratios, and endpoint setup.
What equation should I use for a titration?
Use M₁V₁ = M₂V₂ for 1:1 reactions. If the balanced equation is not 1:1, use n₁M₁V₁ = n₂M₂V₂ so the stoichiometric coefficients are included.
What is the difference between endpoint and equivalence point?
The equivalence point is the stoichiometric point in the reaction. The endpoint is the observed signal, such as an indicator color change, that should be as close to the equivalence point as possible.
Should I enter the initial burette reading or delivered volume?
Use the delivered volume, which is the final burette reading minus the initial reading.
Can I use this calculator for weak acid or weak base titrations?
Yes, if you already know the balanced reaction and only need the stoichiometric concentration or volume calculation. Use a separate pH or buffer tool when you need curve behavior.
How do I handle polyprotic acids?
Use the balanced equation for the specific neutralization step you are calculating and enter the correct stoichiometric coefficients.
How precise should my titration answer be?
Match the precision of your burette readings and standard solution values. For most lab work, report using appropriate significant figures rather than every decimal place shown by the calculator.
References and Further Reading
For more in-depth information about titration, analytical chemistry, and related topics, consult these authoritative sources:
| Resource | Description | Category |
|---|---|---|
| ChemLibreTexts: Analytical Chemistry | Open analytical chemistry material covering acid-base titrations and stoichiometric calculations | Analytical Chemistry |
| Harris, D. C. (2016). Quantitative Chemical Analysis | Comprehensive textbook on analytical chemistry and titrations | Textbook |
| Skoog, D. A., et al. (2013). Fundamentals of Analytical Chemistry | Detailed coverage of titration methods and calculations | Textbook |
| Brown, T. L., et al. (2017). Chemistry: The Central Science | Comprehensive textbook covering acid-base chemistry and titrations | Textbook |