Titration Concentration
Calculator
Results
- Analyte concentration (mol/L)
- 0.094
- Moles of analyte (mol)
- 0.00235
- Moles of titrant (mol)
- 0.00235
Chemistry results
| Analyte concentration (mol/L) | 0.094 |
| Moles of analyte (mol) | 0.00235 |
| Moles of titrant (mol) | 0.00235 |
formula-map diagram
- Analyte concentration (mol/L)
- 0.094
- Moles of analyte (mol)
- 0.00235
- Moles of titrant (mol)
- 0.00235
Formula breakdown
Formula
Ca = (Ct × Vt × ratio) ÷ Va= 0.094
Note
Simplified model: these results assume ideal behaviour (ideal gases, dilute solutions, complete reactions) and standard textbook constants. Real laboratory values vary with temperature, pressure, purity and activity coefficients. Do not rely on this for safety-critical or analytical work.
More in Chemistry
See all →Frequently asked questions
How does titration let you calculate an unknown concentration?+
Titration measures the exact volume of a solution of known concentration (the titrant) needed to completely react with a solution of unknown concentration, and the mole ratio from the balanced equation lets you back-calculate the unknown concentration from moles of titrant used.
What is the equivalence point versus the endpoint in a titration?+
The equivalence point is the theoretical moment when moles of acid exactly equal moles of base (or the stoichiometric ratio is satisfied), while the endpoint is the practically observed moment, usually a color change from an indicator, that's used to estimate it. A well-chosen indicator makes the endpoint very close to the true equivalence point.
How is the unknown concentration formula derived for a simple acid-base titration?+
For a 1:1 reaction, moles of acid equal moles of base at equivalence, so Ca x Va = Cb x Vb, and you solve for whichever concentration is unknown. For reactions with a different mole ratio, that ratio must be included in the equation.
Why does the mole ratio from the balanced equation matter in titration calculations?+
Not all acid-base reactions occur in a simple 1:1 ratio — for example, sulfuric acid (H2SO4) reacting with sodium hydroxide needs two moles of NaOH per mole of acid, so ignoring the stoichiometric ratio will give a concentration that's off by that same factor.
What causes titration results to be inaccurate?+
Common sources of error include overshooting the endpoint (adding titrant past the true equivalence point), an improperly calibrated burette, or an indicator that changes color at a pH different from the true equivalence point. Careful, dropwise addition near the expected endpoint minimizes this error.