What is Precipitation Titration?

Last Update: 18 November 2025

This is part of the HSC Chemistry course under the Module 8 Section 1: Analysis of Inorganic Compounds.

conduct investigations and/or process data involving: gravimetric analysis and precipitation titrations

This video explores what precipitation titration is, specifically, Mohr's and Volhard's method of precipitation titration.

Precipitation titration is a titration method in which a precipitate is formed. It is a quantitative analytic technique that determines the amount of the analyte by measuring volume.

Mohr’s method uses AgNO₃ as the titrant (burette) and a small quantity of yellow potassium chromate (K₂CrO₄) as the indicator to determine the concentration of chloride in a given sample.
- For Mohn's method, the titrant is titrated against a supply of chloride ions such that silver chloride and silver chromate will precipitate
- Despite having a lower K_sp value, silver chromate is more soluble than silver chloride, so the latter will precipitate first

$$K_{sp}(AgCl) = 1.77 \times 10^{-10}$$

$$K_{sp} (Ag_2Cr_2O_4) = 1.2 \times 10^{-12}$$

Mohr’s method also uses a small quantity of K₂Cr₂O₄ (indicator) such that the concentration of silver ions needed to precipitate silver chromate is much greater than that for the precipitation of silver chloride

Silver nitrate is titrated against chloride ions to produce a white precipitate (AgCl). This turns the solution from an initial yellow colour to a beige appearance

$$AgNO_3(aq) + Cl^-(aq) \rightarrow AgCl(s) + NO_3^-(aq)$$

When all chloride ions in a given sample has all been converted to AgCl, additional AgNO₃ reacts with yellow K₂CrO₄(indicator) to produce reddish brown precipitate Ag₂CrO₄.

$$AgNO_3(aq) + K_2CrO_4(aq) \rightarrow AgCl(s) + NO_3^-(aq)$$

Endpoint is reached when the reddish brown colour remains ‘stable’ – does not disappear with stirring.

Left to right: (1): Cl^– and CrO₄^2– only, (2): formation of AgCl(s), (3): formation of Ag₂CrO₄(s)

Disadvantage of Mohr’s method: can only be carried out between pH of 7 and 10. In acidic environments, chromate (CrO₄^2–) is converted to chromic acid which does not react with excess silver ions. Furthermore, the low concentration of chromate ions in solution is not sufficient to precipitate with silver.

Volhard’s method uses titrants other than AgNO₃g. NH₄SCN, and Fe(NO₃)₃ as the indicator to determine the concentration of chloride in a given sample.
- Known excess quantity of AgNO₃ is first mixed with the chloride solution e.g. NaCl. This is placed in the conical flask.

$$AgNO_3(aq) + Cl^-(aq) \rightarrow AgCl(s) + NO_3^-(aq)$$

Excess unreacted AgNO₃ is titrated against NH₄SCN (burette) in the presence of Fe(NO₃)₃ (conical flask).

$$Ag^+(aq) + SCN^-(aq) \rightarrow AgSCN(s)$$

When all of the excess AgNO₃ have reacted with the NH₄SCN, NH₄SCN will start to react with Fe(NO₃)₃ in the conical flask. This produces a blood red complex iron(III) thiocyanate (FeSCN²⁺). The red colour will mix with the original yellow appearance to make the solution seem orange (centre flask). When this orange colour remains ‘stable’, endpoint is reached.

$$Fe^{3+}(aq) + SCN^-(aq) \rightarrow FeSCN^{2+}(aq)$$

Volhard’s method is a variant of back titration. The endpoint indicated by the formation of iron(III) thiocyanate first determines the amount of excess unreacted Ag⁺. Thus:

number of moles of Cl^- =initial mole of AgNO₃ – unreacted AgNO₃

Volhard’s method is used if the pH of the solution in the conical flask is acidic. If the solution is neutral or basic, Mohr’s method should be used.