H₃O⁺ + OH⁻ → 2 H₂OIonic neutralization reaction between species in solution.
Use when: This writing describes the strong acid–strong base step; weak acids require their own balance.
Acid–base titrations
Determine the concentration of an acid or a base using a neutralization reaction.
What is happening?
The titrant of known concentration is added gradually to the test portion. At equivalence, the quantities introduced respect the stoichiometry of the reaction.
The jump in pH makes it possible to identify the equivalence. The turning point of an indicator must be close to this zone; a pH equal to 7 is not a general rule for all titrations.
The formulas, with their conditions.
cₐVₐ / a = cᵦVₑ / ba A + b B → products; c to mol/L ; V in the same unit.
Use when: Relationship to equivalence for a quantitative and sufficiently rapid reaction.
pH = −log₁₀(aH₃O⁺)aH₃O⁺: dimensionless activity.
Use when: In dilute solution, aH₃O⁺ ≈ [H₃O⁺]/(1 mol/L).
Where is this principle used?
Food factory
Control the acidity of drinks and raw materials.
Water treatment
Measure acidity or alkalinity.
What to observe in the experiment
Compare the curves of a strong acid and a weak acid with the same initial quantity. Look for the pH jump, not an imposed pH value.
References and readings
This sheet explains the principles and their assumptions. Educational simulation can simplify the process; an industrial model requires suitable data and validation.
Have you understood the essentials?
Only one correct answer per question. Answer all three questions, then view the answer key.
Intu Lab · Understanding sheet · Kimba Christian