Acid-Base Titration: Experimental Procedure and Error Analysis | 酸碱滴定实验操作与误差分析

📚 Acid-Base Titration: Experimental Procedure and Error Analysis | 酸碱滴定实验操作与误差分析

Acid-base titration is a fundamental technique in quantitative chemistry, where a solution of known concentration (the titrant) is added from a burette to a measured volume of an analyte until the equivalence point is reached. The volume of titrant consumed allows the concentration of the analyte to be calculated with high precision. This article covers the essential experimental procedures and a thorough analysis of common errors.

酸碱滴定是定量化学中的一项基本技术，将已知浓度的溶液（滴定剂）从滴定管加入装有已知体积待测液的锥形瓶中，直至达到等当点。根据消耗的滴定剂体积，可高精度计算出待测液浓度。本文将全面介绍核心实验操作流程与常见误差分析。

1. Fundamental Principle and Definitions | 基本原理与定义

The titration relies on a complete neutralisation reaction between an acid and a base: H⁺ + OH⁻ → H₂O. The equivalence point is reached when the added moles of titrant are exactly stoichiometrically equivalent to the moles of analyte present. For a monoprotic acid and monobasic base, this occurs when n(acid) = n(base).

滴定基于酸碱之间的完全中和反应：H⁺ + OH⁻ → H₂O。当加入的滴定剂摩尔数与待测物摩尔数恰好满足化学计量关系时，即达到等当点。对于一元酸与一元碱，此时 n(酸) = n(碱)。

c(analyte) = c(titrant) × V(titrant) ÷ V(analyte)

The endpoint is the point at which the indicator changes colour, indicating that the equivalence point has been reached. Ideally, the endpoint coincides exactly with the equivalence point.

终点是指示剂发生颜色变化的时刻，表明已到达等当点。理想情况下，终点应与等当点完全重合。

2. Essential Apparatus and Their Roles | 必备仪器及其作用

The core apparatus includes a burette (50.00 cm³, readable to ±0.05 cm³), a volumetric pipette (typically 25.00 cm³, accurate to ±0.06 cm³), a conical flask, a white tile, a funnel, and a clamp stand. The burette delivers the titrant, the pipette transfers a fixed volume of analyte, and the conical flask holds the analyte during titration.

核心仪器包括滴定管（50.00 cm³，可读

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