How to use (3 steps)
- Select the titration type (strong/weak) and enter the concentrations and volumes.
- Choose a single-point pH or generate the full titration curve range.
- Tap Compute to view pH, regions (buffer/equivalence), and the calculation steps. Copy URL shares the exact setup. The results card below shows the curve and table.
A weak acid + strong base example is prefilled so you can compute immediately and review the pH summary, curve, and steps together.
Inputs
Calculation mode
Results
How it's calculated
How to read the titration result
Start with the titration type, concentrations, and initial volume. Then decide whether you need one pH point or the full curve. Keep the first run as your baseline before you compare any other setup.
What to check before computing
Use the same concentration units for analyte and titrant, and make sure the weak-acid/weak-base constant matches the selected titration type. If the curve range is too short, you may miss the equivalence region.
How to interpret the output
Read the region label together with the pH and the step list. Before equivalence, buffer logic may dominate. Near equivalence, the conjugate species matters more. After equivalence, excess titrant usually controls the pH.
Common mistakes to avoid
- Changing both chemistry type and concentrations at the same time, which makes the pH shift harder to explain.
- Entering pKa when the selected mode expects pKb, or the reverse.
- Comparing two runs without checking that the added-volume range is the same.
- Reading only the final pH without checking the step-by-step region change.
See also
FAQ
What assumptions does this titration calculator make?
It assumes monoprotic strong/weak acids and bases at 25 °C with ideal behaviour. Polyprotic species, activity coefficients, ionic strength, and temperature dependence are out of scope for this tool.
Does the equivalence point always give pH 7?
For strong acid and strong base, the equivalence point is near pH 7 at 25 °C. For weak acid with strong base, the conjugate base is present at equivalence, so the pH will be above 7.
When is the Henderson-Hasselbalch equation valid?
It is a good approximation before the equivalence point while both the acid/base and its conjugate are present. Near or after equivalence, this calculator switches to expressions for the dominant species.
Why can the equivalence-point pH change between titration types?
Strong acid/strong base titrations tend to sit near pH 7 at equivalence, while weak systems inherit conjugate-acid or conjugate-base effects that shift the equivalence pH above or below 7.
Practical interpretation checklist
Before equivalence
If both the weak species and its conjugate are present, the buffer region usually explains the pH trend. Use the step list to confirm when the page switches into that approximation.
At equivalence
Do not assume pH 7 automatically. Strong acid plus strong base is the simple case; weak systems can shift the equivalence pH above or below 7.
After equivalence
Check whether the result is now controlled by excess titrant. A sudden pH jump is expected if the final segment is dominated by strong acid or strong base left over after neutralization.
When a result feels wrong
Recheck units, constants, and the selected chemistry mode first. Then compare the exact added volume and equivalence volume instead of comparing only the final pH label.
Related calculators
- Acid-base titration curve simulatorPlot the full titration curve directly when you want a dedicated curve-first view with the same chemistry family.
- Acid–base pHCheck a single acid/base mixture or concentration setup before moving into the full titration workflow.
- Beer-Lambert law & calibration curveContinue with another chemistry workflow that pairs numeric output with calibration or interpretation steps.
- Buffer pH (Henderson-Hasselbalch)Focus on the buffer-region approximation alone when you want to inspect Henderson-Hasselbalch behaviour without the full titration curve.
- Concentration & pH Calculator (Step-by-Step)Recheck molarity and pH assumptions before comparing titration runs or preparing a fresh solution.
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