Titration Simulator
Interactive simulation — adjust parameters and watch the visualization update in real time.
Flask + indicator
1.00
Acidic
V_a = 25 mL · C_a = 0.10 M · C_b = 0.10 M · V_b = 0.00 mL
Burette
0.0 mL
Live graphs
How it works
Add **strong base** from a burette into a flask of **acid**. The **pH curve** shows how pH changes with titrant volume. For **strong–strong** titrations the equivalence point is at **pH 7**. For **weak acid / strong base**, the equivalence region is **basic** because the conjugate base hydrolyzes. Use **Jump to V_eq** to land on the stoichiometric point.
Key equations
Strong–strong: [H⁺] = (C_a V_a − C_b V_b) / (V_a + V_b) before equivalence; after, use [OH⁻] similarly. At C_a V_a = C_b V_b → pH 7.
Weak acid buffer: pH = pK_a + log([A⁻]/[HA]). At equivalence: [OH⁻] ≈ √(K_b · [A⁻]).