1. Inorganic and Analytical Chemistry
Gravimetric Analysis
Inorganic and Analytical Chemistry
PE-214
Dr. Riham Hazzaa

2. Gravimetric Analysis: is based upon the measurement of mass
Gravimetric Analysis generalized into two types: precipitation and volatilization
(i ) A technique in which the amount of an analyte in a sample is determined by converting the analyte to some product
Mass of product can be easily measured
(ii) Analyte: the compound or species to be analyzed in a sample
Advantages -
requires minimal equipment
Disadvantage –
requires skilled operator,
slow.
Dr.Riham Hazzaa

3. precipitation reaction, filtering,
The quantitative determination of a substance by the precipitation method of gravimetric analysis involves isolation of an ion in solution by:
precipitation reaction,
filtering,
washing the precipitate free of contaminants, conversion of the precipitate to a product of known composition,
drying
weighing the precipitate and determining its mass by difference. 
Dr.Riham Hazzaa

4. Reaction of potassium iodide solution and lead (II) nitrate solution.
Precipitation
Determination of lead (Pb+2) in water
Reaction of potassium iodide solution and lead (II) nitrate solution.
Dr.Riham Hazzaa

5. Determination of lead (Pb+2) in water
Pb Cl-  PbCl2(s)
By adding excess Cl- to the sample, essentially all of the Pb+2 will precipitate as PbCl2.
Mass of PbCl2 is then determined.
used to calculate the amount of Pb+2 in original solution
Analyte
Reagent
Solid Product
Dr.Riham Hazzaa

6. Mechanism of precipitation
Induction period time between mixing and visual appearance of a precipitate called the induction period
Nucleation is the formation, in a super saturation solution, of the smallest aggregate of molecules capable of growing into a large precipitate particle.
Dr.Riham Hazzaa

7. Crystal growth Once a nucleation aggregate has formed, it begins to grow as ions or molecules from the solution deposit on the surface in a regular, geometric pattern.
Aggregate growth Natural cohesive forces exist between particles having the same composition and, as a result, most precipitate to consist of a relatively few large aggregate of crystals.
Crystal Growth
Dr.Riham Hazzaa

8. Why colloids occur??
Dr.Riham Hazzaa

9. How colloidal suspension is prevented????
Keep the volume of the counter ion layer small:
Keep the charge of the primary adsorption layer small by avoiding an excess of the precipitating ion.
Increase the ionic strength by adding soluble electrolyte.
Heating and stirring reduces the volume of the electrical double layer. This will allow the ions in the counter ion layer be closer to the opposite charged ions of the primary layer.
Dr.Riham Hazzaa

10. Desired Properties of Solid Product Should be very insoluble
Easily filterable (i.e., large crystals)
Very Pure
Known and constant composition
Few precipitates have all of these properties, but in most cases appropriate techniques can help optimize these qualities
Dr.Riham Hazzaa

11. The solubility of a precipitate can be decreased by:
Decreasing temperature of solution
Using a different solvent
- usually a less polar or organic solvent (likes dissolves likes)
Solubility vs. pH
Solubility vs. Common Ion Effect
Solubility vs. Temperature
Dr.Riham Hazzaa

12. Filterability: product be large enough to collect on filter:
Doesn’t clog filter
Doesn’t pass through filter
Best Case: Pure Crystals
Worst Case: Colloidal suspension
Difficult to filter due to small size
Tend to stay in solution indefinitely  suspended by Brownian motion
usually nm in size
Dr.Riham Hazzaa

13. Conditions for analytical precipitation
An analytical precipitate for gravimetric analysis should consist of perfect crystals large enough to be easily washed and filtered. The perfect crystal would be large and free from impurities. The precipitate should also be "insoluble".
Want to
Convert to
Crystal formation
Colloidal suspension
Dr.Riham Hazzaa

14. Relative supersaturation =
It has been shown that the particle size of precipitates is inversely proportional to the relative supersaturation of the solution during precipitation;
  Relative supersaturation =
S = concentration of solute in solution at equilibrium
Q = actual concentration of solute added to solution
Dr.Riham Hazzaa

15. Methods used to improve particle size and filterability
Precipitation from hot solution The solubility S of precipitates increases with temperature and so an increase in S decreases the supersaturation.
Precipitation from dilute solution  This keeps Q low. Slow addition of precipitating reagent with effective stirring. This also keeps Q low; stirring prevents local high concentrations of the precipitating agent.
Precipitation at a pH near the acidic end of the pH range Many precipitates are more soluble at the lower (more acidic) pH values and so the rate of precipitation is slower.
Digestion of the precipitate. Heating the precipitate in the precipitating solution, a process called digestion, results in larger and purer particles by giving the crystal a chance to dissolve and reprecipitate.

16. Impurities in Precipitates
Impurities can be incorporated into a precipitate during its formation, called co-precipitation, or after its formation while still in contact with the precipitating solution, called postpricipitation
Co-precipitation
a) Surface adsorption
Dr.Riham Hazzaa

17. c) Inclusion Impurities placed in the crystal instead of analyte
b) Occlusion Impurities absorbed or trapped within pockets in the crystal
c) Inclusion Impurities placed in the crystal instead of analyte
Dr.Riham Hazzaa

18. It must be capable of drying or of ignition.
There are several requirements that must be met to make precipitation reliable:
The precipitate must have a very low solubility in water; i.e. its Ksp must be very small number
It must precipitate in a high state of purity or be capable of reprecipitation for further purification.
It must be capable of drying or of ignition.
It should not be hydroscopic at room temperature.
Dr.Riham Hazzaa

19. Ageing &digestion
The precipitate should be in contact with the solution from which the precipitate is formed.
Warm the solution that contains the precipitate for some time to obtain complete precipitation in a form which can be readily filtered.
Dr.Riham Hazzaa

20. During the process of ageing and digestion, two changes occur:
After precipitation has occurred, the very small particles, which have a greater solubility than the greater ones, tend to pass into solution and will redeposit upon the larger particles. Thus co precipitation on the minute particles is eliminated.
The rapidly formed crystals are irregular. Thus on ageing they will become regular and the surface area is reduced, so adsorption will be reduced. The net result of digestion is usually to reduce the extent of co precipitation and to increase the size of the particles, rendering filtration easier.
Dr.Riham Hazzaa

21. Filtration A precipitate may be separated by filtering it through
paper,
sintered glass,
or sintered porcelain.
The choice depends on the nature of the precipitate and on the temperature to which it will be heated after filtering.
Dr.Riham Hazzaa

22. Washing
The precipitate and filter must be washed with suitable electrolyte to remove dissolved solids that remain in the precipitate and wetted filter.
Problems with coprecipitation and surface adsorption may be reduced by careful washing of the precipitate.
With many precipitates, peptization occurs during washing.
Dr.Riham Hazzaa

23. Precipitates from ionic compounds
- need electrolyte in wash solution TO keep precipitate from breaking up and redissolving (peptization)
Electrolyte should be volatile removed by drying
- HNO3, HCl, NH4, NO3, etc.
Example:
AgCl(s) should not be washed with H2O, instead wash with dilute HNO3
Dr.Riham Hazzaa

24. Drying/Igniting Precipitates
Precipitates are dried at about 120oC for accurate, stable mass measurements
Dr.Riham Hazzaa