Mohr's method: Difference between revisions
(→Method) |
(→Method) |
||
Line 24: | Line 24: | ||
<br/> | <br/> | ||
==Method== | ==Method== | ||
*Preparation of ~1 N original solutions of MgCl<sub>2</sub> and CaCl<sub>2</sub> | *Preparation of ~1 N original solutions of MgCl<sub>2</sub> and CaCl<sub>2</sub> | ||
*Preparation of diluted solutions of MgCl<sub>2</sub> and CaCl<sub>2</sub> (1/20 dilution) | *Preparation of diluted solutions of MgCl<sub>2</sub> and CaCl<sub>2</sub> (1/20 dilution) | ||
*Titration of diluted solutions with standardized silver nitrate solution | *Titration of diluted solutions with standardized silver nitrate solution | ||
*Calculation of the concentration of CaCl<sub>2</sub> and MgCl<sub>2</sub> in the original solutions | *Calculation of the concentration of CaCl<sub>2</sub> and MgCl<sub>2</sub> in the original solutions | ||
*Calculation of the density of CaCl<sub>2</sub> and MgCl<sub>2</sub> original solutions | *Calculation of the density of CaCl<sub>2</sub> and MgCl<sub>2</sub> original solutions | ||
*Calculation of the weight of CaCl<sub>2</sub> and MgCl<sub>2</sub> original solutions (to introduce in the buffer solution) | *Calculation of the weight of CaCl<sub>2</sub> and MgCl<sub>2</sub> original solutions (to introduce in the buffer solution) | ||
<br/> | <br/> | ||
Revision as of 11:10, 15 July 2006
The chloride ion concentration of the MgCl2 and CaCl2 solutions is determined by a precipitation titration with calibrated silver nitrate solution. This procedure is known as Mohr’s method.
Equipment and chemicals
Equipment
- 2 x 200 ml beakers (for MgCl2 and CaCl2 weighing)
- 4 x 100 ml beakers (for pipet rinsing)
- 6 x 100 ml beakers (for MgCl2 and CaCl2 density determination)
- 2 x 500 ml volumetric flasks (for original solutions)
- 2 x 100 ml volumetric flasks (for diluted solutions)
- 1 x 5 ml automatic pipet
- 1 x 25 ml volumetric pipet
- 1 x 50 ml buret
- 6 x 50 ml Erlenmeyer flasks
- 6 x small magnetic stir bars
- 2 x funnels (for powder of MgCl2 and CaCl2 original solutions)
Chemicals
- Distilled water
- MgCl2 (+6H2O)
- CaCl2 (+2H2O)
- AgNO3 0.1 N (Standardized silver nitrate solution)
- NaHCO3
- K2Cr2O7 (1.25 g K2Cr2O7 dissolved in 25 ml distilled water)
Method
- Preparation of ~1 N original solutions of MgCl2 and CaCl2
- Preparation of diluted solutions of MgCl2 and CaCl2 (1/20 dilution)
- Titration of diluted solutions with standardized silver nitrate solution
- Calculation of the concentration of CaCl2 and MgCl2 in the original solutions
- Calculation of the density of CaCl2 and MgCl2 original solutions
- Calculation of the weight of CaCl2 and MgCl2 original solutions (to introduce in the buffer solution)
Detailed protocol
Preparation of ~1 N original solutions of MgCl2 and CaCl2
500 ml MgCl2’’<br/
(MgCl2.6 H2O = 203 g/mol)
101.65 g MgCl2 dissolved in distilled water in 500 ml volumetric flask, make it up to the mark with distilled water.
Mix the solution up to total dilution
500 ml CaCl2<br/
(CaCl2.2 H2O = 147.02 g/mol)
- 73.51 g CaCl2 dissolved in distilled water in 500 ml volumetric flask, make it up to the mark with distilled water.
- Be careful, the distilled water must be added little by little since the reaction emanate a lot of warmth. *Mix the solution up to total dilution and wait for cooling.
Preparation of ~0.05 N diluted solutions of MgCl2 and CaCl2
- Dilute original solutions of MgCl2 and CaCl2 by a factor 20 by taking 5 ml of original solution with an automatic pipet, pipetting it into a 100 ml volumetric flasks, and making it up to the mark with distilled water.
- N.B. Pour a part (~20 ml) of the original solution of MgCl2 and CaCl2 in 2 beakers rather than pipetting directly in the volumetric flasks.
Titration of diluted solutions with standardized silver nitrate solution
- Pipette a 25 ml aliquot of diluted solutions of MgCl2 and CaCl2 (with 25 ml volumetric pipets) into 50 ml Erlenmeyer flasks (3 replicates for each solution).
- Add magnetic stir bars.
- Add a pinch of NaHCO3 and some drops (2-3 drops) of K2Cr2O7 indicator (diluted potassium chromate solution) in the erlenmeyer flasks.
- Fill the 50 ml buret with the 0.1 N silver nitrate solution.
- Titrate the diluted solution of MgCl2 and CaCl2 with the silver nitrate solution (a drop at a time) up to the first appearance of a red-brown color (Fig. 1)
Figure 1. Flasks before the titration endpoint (left) and at the endpoint (right)
- Use the mean of the 3 titrations as a final result.
Calculation of the normality of CaCl2 and MgCl2 in the original solutions
- Calculate the average volume of AgNO3 used for the titration of the three replicates of diluted solution: AgNO3 volume (0.1 N) = V
- Calculate the amount (in moles) of AgNO3 reacting: x = V*0.1 mole
- Calculate the amount (in moles) of chloride ions reacting:
- for 25 ml of diluted solution: x/2 mol MgCl2 et CaCl2
- for 1 l of diluted solution : x/2 * 40 mol MgCl2 et CaCl2
- for 1 l of original solution: x/2 * 40 *20 mol MgCl2 et CaCl2
Original solution normality (mol/l)= (V * 0.1 / 2) * 40 * 20 / 1000
Calculation of the density of CaCl2 and MgCl2 in the original solutions
Weigh at least 3 aliquots of 20 ml of original solution in beakers and calculate the average weight (W, g)
Density (g/ml) = W / 20
Calculation of the weight of original CaCl2 and MgCl2 solution for ½ l of buffer solution
Weight (g) = ((molarity / normality) * density * 1000) / 2
Molarity = 0.05474/2 mol MgCl2 and 0.01075/2 mol CaCl2 for ½ l of buffer solution