Gravimetric Gravimetric methods o f analysis analysis Gravimetry Gravimetric methods are quantitative methods that are based on determining the mass of a pure compound to which the analyte is chemically related.
Classifications of Gravimetric methods 1-Precipitation gravimetry, the analyte is separated from a solution of the sample as a precipitate and is converted to a compound of known composition that can be weighed. 2-Volatilization gravimetry, the analyte is separated from other constituents of a sample by conversion to a gas of known chemical composition. The weight of this gas then serves as a measure of the analyte concentration. 3-Electrogravimetry, the analyte is separated by deposition on an electrode by an electrical current. The mass of this product then provides a measure of the analyte concentration. Features Features or properties of Gravimetric Gravimetric Analysis · · · · · ·
Traditional Tradit ional Method. Cheap, easily available apparatus, simple to carry out. Slow, especially when accurate results are required. Wide range of sample concentrations concentrations (ng - kg). No calibration required (except for the balance). Accurate.
Precipitation Gravimetry In precipitation gravimetry, the analyte is converted to a sparingly soluble precipitate. This precipitate is then filtered, washed free of impurities, converted to a product of known composition by suitable heat treatment, and weighed. For example, a precipitation method for determining calcium in natural waters. The reactions are: 2NH3 + H2C2O4 Ca+2 (aq) + C2O4-2 (a (aq)
2NH4++C2O4-2 CaC2O4 (s)
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The precipitate is filtered using a weighed filtering crucible, then dried and ignited. The process converts the precipitate entirely to calcium oxide. The reaction is: CaC2O4 (s)
Δ
CaO (s) + CO (g) + CO2
After cooling, the crucible and precipitate are weighed, and the mass of calcium oxide is determined by subtracting the known mass of the crucible. The calcium content of the sample is then computed.
Procedure for gravimetric analysis analysis (Precipitati (Precipitati on gravimetr y) What steps are needed? needed? The steps required in gravimetric analysis, after the sample has been dissolved, can be summarized as follows: 1. 2. 3. 4. 5. 6. 7. 8.
Preparation of the sol ution Precipit ation Digesti on Filtration W ashing sample Drying or igniting W eighing Calcul ation
dissolved components
precipitating precipitating agent
Properties of precipi tates and precipit ating reagents reagents Properties Properties precipitating reagents reagents
Ideally, a gravimetric precipitating agent should react specifically or at least selectively with the analyte. Specific reagents, which are rare, react only with a single chemical species. Selective reagents, which are more common, react with a limited number of species.
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Properties of good pr ecipitates
1. Easily filtered and washed free of contaminants. 2. Of sufficiently low solubility that no significant loss of the analyte occurs during filtration and washing. 3. Unreactive with constituents of the atmosphere 4. Of known chemical composition after it is dried or, if necessary, ignited.
Part icle size and filterabilit y of precip itates Why we prefer pr ecipitates of large particles.
Precipitates consisting of large particles are generally desirable for gravimetric work because these particles are easy to filter and wash free of impurities. In addition, precipitates of this type are usually purer than are precipitates made up of fine particles.
Factor s th at determin e the partic le size of p recipit ates The particle size of solids formed by precipitation varies enormously.
1-Colloidal suspensions, ·
whose tiny particles are invisible to the naked eye (10-7 _ 10-4 cm in diameter).
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C olloidal pa rticles show no tendenc y to settle from solution
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not easily filtered.
2-Cryst alline suspension ·
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partic les with dimensions on the order of tenths of a millimeter or greater. The temporary dispersion of such particles of a tend to settle spontaneously, ea sily filtered.
Scientists have studied precipitate formation for many years, but the mechanist of the process is still not fully understood. It is certain, however, that the particle size of a precipitate is influenced by such experimental variables as precipitate solubility, temperature, reactant 3
concentrations, and rate at w hic h reactants are mix ed. The net effect of these variables can be accounted for, at least qualitatively, by assuming that the particle size is related to a single property of the system called the relative supersaturations , where:
in this equation, Q is the concentration of the solute at any instant and S is tits equilibrium solubility. Generally, precipitation reactions are slow, so that even when a precipitating reagent is added drop by drop to a solution of an analyte, some s supersaturation is likely. Experimental evidence indicated that the particle size of a precipitate varies inversely with the average relative supersaturation during the time when the reagent is being introduced. Thus, when (Q _ S)/S is large, the precipitate tends to be colloidal, when (Q _ S)/S is small, a crystalline solid is more likely. High relative supersaturation
many small crystals (high surface area)
Low relative supersaturation
fewer, larger crystals (low surface area)
Obviously, then, we want to keep Q low and S high during precipitation. Several steps are commonly taken to maintain favorable conditi ons for precipi tation or t he experimental contro l of particle size 1. Precipitate from dilute solution. This keeps Q low. 2. Add dilute precipitating reagents slowly, with effective stirring, this also keeps Q low. Stirring prevents local excesses of the reagent. 3. Precipitate from hot solution. This increase S. the solubility should not be too great or the precipitation will not be quantitative (with less than 1 part per thousand remaining). The bulk of the precipitation may be performed in the hot solution, and then the solution may be cooled to make the precipitation quantitative. 4. Precipitate at as low a pH as is possible to maintain quantitative precipitation. As we have seen, many precipitates are more soluble in acid medium, and this slows the rate of precipitation. They are more soluble because the anion of the precipitate combines with protons in the solution.
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Colloidal Precipitates Individual colloidal particles are so small that they are not retained by ordinary filters. Moreover, Brownian motion prevents their settling out of solution under the influence of gravity. Fortunately, however, we can coagulate, or agglomerate, the individual particles of most colloids to give a filterable, amorphous mass that will settle out of solution.
Structure of Colloids Colloidal suspensions are stable because all of the particles of the colloid are either positively or negatively charged. Colloidal particles are very small and have a very large surface-to-mass ratio, which promotes surface adsorption. (The process by which ions are retained on the surface of a solid is known as adsorption). As a precipitate forms, the ions are arranged in a fixed pattern. In AgCl, for example, there will be alternating Ag + and Cl- ions on the surface. While there are localized (+) and (-) charges on the surface, the net surface charge is zero. However, the surface does tend to adsorb the ion of the precipitate particle that is in excess in the solution, for example, Cl - if precipitating Cl- with Ag+; this imparts a charge. (With crystalline precipitates, the degree of such adsorption will generally be small in comparison with particles that tend to form colloids.) The adsorption creates a primary layer that is strongly adsorbed and is an integral part of the crystal. It will attract ions of the opposite charge in a counter layer(counter-ion layer) or secondary layer so the particle will have an overall neutral charge. There will be solvent molecules interspersed between the layers. Normally, the counter layer completely neutralizes the primary layer and is close to it, so the particles will collect together to form largersized particles; that is, they will coagulate. However, if the secondary layer is loosely bound, the primary surface charge will tend to repel like particles, maintaining a colloidal state.
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A col loid al s il ver chlo rid e part ic le sus pen ded in a s ol ut ion of si lver nitrat e.
Coagulation of Colloids Coagulation of a colloidal suspension can often be brought 1.by short period of heating to decreases the number of adsorbed ions and thus the thickness, of the double layer. 2.Increase the electrolyte concentration of the solution.
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If we add ionic compound to a colloidal suspension. The concentration of counter – ions increases in the vicinity of each particle. The net effect of adding an electrolyte is thus a shrinkage of the counter-ion layer.
Pepti zation of Coll oid s Peptization is the process by which a coagulated colloid reverts to its original dispersed state. Peptization is the reverse of coagulation (the precipitate reverts to a colloidal state and is lost). It is avoided by washing with an electrolyte that can be volatized by heating.
Practical Treatment of Colloi dal Precipitates Colloids are best precipitated from hot. stirred solutions containing sufficient electrolyte to ensure coagulation. The filterability of a coagulated colloid frequently improves if it is allowed to stand for an hour or more in contact with the hot solution from which it was formed. This process is known as digestion.
Digestion is a process in which a precipitate is heated for an hour or more in the solution from which it was formed (the mother liquor).
Crystalline Precipitates Crystalline precipitates are generally more easily filtered and purified than are coagulated colloids. In addition, the size of individual crystalline particles, and thus their filterability, can be controlled to a degree.
Mechanism o f Precipitate Formation The effect of relative supersaturation on particle size can be explained if we assume that precipitates form in two ways, by: nucleation and by particle growth. The particles size of a freshly formed precipitate is determined by the mechanism of predominates. After the addition of the precipitating agent to the solution of the ion under analysis there is an initial induction period before nucleation occurs. This induction period may range from a very short
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time period to one which is relatively long, ranging from almost instantaneous to several minutes. In nucleation, a few ions, atoms, or molecules (perhaps as few as four or five) come together to form a stable solid.
Often, these nuclei form on the surface of suspended solid contaminants, such as dust particles. Further precipitation then involves a competition between additional nucleation and growth on existing nuclei (particle growth). ·
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If nucleation predominates, a precipitate containing a large number of small particles results, If growth predominated, a smaller number of larger particles is produced.
We can summarized the precipitation mechanism 1) Induction period. 2) Nucleation. 3) Particle growth to form larger crystal 4) Adsorption. 5) Electrostatic.
Impurities in Precipit ates Precipitates tend to carry down from the solution other constituents that are normally soluble, causing the precipitate to become contaminated. This process is called coprecipitation. In other wards, coprecipitation is a phenomenon in which otherwise soluble compounds are removed from solution during precipitate formation.
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There are four types of coprecipitation: 1.surface adsorption, 2.mixed-crystal formation, 3.occlusion, 4. mechanical entrapment.
A
B
C
D
Types of coprecipitation: A: surface adsorption B: inclusion-isomorphic carrying (Mixed-crystal formation) C: occlusion D: mechanical entrapment in colloidal.
1- Surface adsor ptio n Adsorption is a common source of coprecipitation and is likely to cause significant contamination of precipitates with large specific surface areas, that is, coagulated colloids. Although adsorption does occur in crystalline solids, its effects on purity are usually imdetectable because of the relatively small specific surface area of these solids. The net effect of surface adsorption is therefore the carrying down of an otherwise soluble compound as a surface contaminant. In order to minimizing adsorbed impurities on colloids:
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Using digestion process to improve the purity. Washing a coagulated colloid with a solution containing a volatile electrolyte. The adsorbed layers can often be removed by washing. Reprecipitation is effective way to minimize the effects of adsorption.
2- Mixed-cr ystal fo rmation Mixed-crystal formation ,one of the ions in the crystal lattice of a solid is replaced by an ion of another element. For this exchange to occur, it is necessary that the two ions have the same charge and that their sizes differ by no more than about 5%. This problem occur with both colloidal suspensions and crystalline precipitates. Ex (Pb ion replace some of the barium ion). In order to minimizing this type of coprecipitation: ·
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the interfering ion may have to be separated before the final precipitation step. a different precipitating reagent that does not give mixed crystals with the ions interested may be used.
3- Occlusio n Occlusion is a type of coprecipitation in which a compound is trapped within a pocket formed during rapid crystal growth. , material that is not part of the crystal structure is trapped within a crystal. For example, water may be trapped in pockets when AgN0 3 crystals are formed. Occluded impurities are difficult to remove. Digestion may help some but is not completely effective. The impurities cannot be removed by washing. Reprecipitation that go on at the elevated temperature of digestion open up the pockets and allow the impurities to escape into the solution.
4- Mechanical entr apment Mechanical entrapment occurs when crystals lie close together during growth. Here, several crystals grow together and in so doing trap a portion of the solution in a tiny pocket. Mechanical entrapment can be minimumize when the rate of precipitate formation is low—that is under conditions of low supersaturation. In addition, digestion is often remarkably helpful in reducing this types of coprecipitation.
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Precipitation from Homogeneous Solution Precipitation from homogeneous solution is a technique in which a precipitating agent is generated in a solution of the analyte by a slow chemical reaction. Local reagent excesses do not occur because the precipitating agent appears gradually and homogeneously throughout the solution and reacts immediately with the analyte. As a result, the relative supersaturation is kept low during the entire precipitation. In general, homogeneously formed precipitates, both colloidal and crystalline, are better suited for analysis than a solid formed by direct addition of a precipitating reagent.
Drying and Ignition of Precipitates After filtration, a gravimetric precipitate is heated until its mass becomes constant. Heating removes the solvent and any volatile species carried down with the precipitate. Some precipitates are also ignited to decompose the solid and form a compound of known composition. This new Compound is often called the weighing f orm.
Types of Precipitating Agents 1- Inorganic Precipitating Agents These reagents typically form slightly soluble salts or hydrous oxides with the analyte. As you can see from the many entries for each reagent, few inorganic reagents are selective.
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2- Reducing Agents This type of reagents convert an analyte to its elemental form for weighing.
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3- Organic Precipitating Agents Numerous organic reagents have been developed for the gravimetric determination of inorganic species. Some of these reagents are significantly more selective in their reactions than the inorganic reagents. We encounter two types of organic reagents. One forms slightly soluble non-ionic products called coordination compounds; the other forms products in which the bonding between the inorganic species and the reagent is largely ionic.
Organic precipitating agents have the advantages of: ·
Some of organic precipitating agents are very selective, and others are very broad in the number of elements they will precipitate.
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giving precipitates with very low solubility in water.
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give a favorable gravimetric factor.
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Calculation of Results from Gravimetric Data The results of a gravimetric analysis are generally computed from two experimental measurements: the mass of sample and the mass of a product of known composition . The precipitate we weigh is usually in a different form than the analyte whose weight we wish to report. The principles of converting the weight of one substance to that of another depend on using the stoichiometric mole relationships. We introduced the gravimetric factor (GF), which represents the weight of analyte per unit weight of precipitate. It is obtained from the ratio of the formula weight of the analyte to that of the precipitate, multiplied by the moles of analyte per mole of precipitate obtained from each mole of analyte, that is,
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In gravimetric analysis, we are generally interested in the percent composition by weight of the analyte in the sample, that is,
We obtain the weight of substance sought from the weight of the precipitate and the corresponding weight/mole relationship
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Calculations are usually made on a percentage basis:
where g A represents the grams of analyte (the desired test substance) and gsampie represents the grams of sample taken for analysis. We can write a general formula for calculating the percentage composition of the substance sought:
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Ap pl ic ation s of Gravimetr ic Metho ds Gravimetric methods have been developed for most inorganic anions and cations, as well as for such neutral species as water, sulfur dioxide, carbon dioxide, and iudine. A variety of organic substances can also be easily determined gravimetri-cally. Examples include lactose in milk products, salkylates in drug preparations, phenolphthalein in laxatives, nicotine in pesticides, cholesterol in cereals, and benzaldehyde in almond extracts. Indeed, gravimetric methods are among the most widely applicable of all analytical procedures
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