Solubility of silver chloride

Though both silver nitrate and sodium chloride have high solubility in water, silver chloride is very slightly soluble. What will happen if we mix a solution of silver nitrate and sodium chloride Then, we will have a solution that includes the species present in a solution of silver chloride, Ag+(aq) and Cl (ag), but now they are present at high concentration The Ag+(agJ came from reaction (8) and the Cl (aq) came from reaction (6) and their concentrations far exceed the solubility of silver chloride. The result is that solid will be formed. The formation of solid from a solution is called precipitation ... [Pg.80]

The solubility of silver chloride is so low that all but a negligible amount of it is precipitated when excess sodium chloride solution is added to silver nitrate solution. What would be the weight of the precipitate formed when 100 ml of 0.5 M NaCl is added to 50.0 ml of 0.100 M AgNOs ... [Pg.178]

The solubility product of AgCl is 1.4 x 10-4 at 100°C. Calculate the solubility of silver chloride in boiling water. [Pg.178]

Example 1. The solubility of silver chloride is 0.0015 g per L. Calculate the solubility product. [Pg.25]

The solubility of the precipitates encountered in quantitative analysis increases with rise of temperature. With some substances the influence of temperature is small, but with others it is quite appreciable. Thus the solubility of silver chloride at 10 and 100 °C is 1.72 and 21.1mgL 1 respectively, whilst that of barium sulphate at these two temperatures is 2.2 and 3.9 mg L 1 respectively. In many instances, the common ion effect reduces the solubility to so.small a value that the temperature effect, which is otherwise appreciable, becomes very small. Wherever possible it is advantageous to filter while the solution is hot the rate of filtration is increased, as is also the solubility of foreign substances, thus rendering their removal from the precipitate more complete. The double phosphates of ammonium with magnesium, manganese or zinc, as well as lead sulphate and silver chloride, are usually filtered at the laboratory temperature to avoid solubility losses. [Pg.30]

Consider now a somewhat different type of complex ion formation, viz. the production of a complex ion with constituents other than the common ion present in the solution. This is exemplified by the solubility of silver chloride in ammonia solution. The reaction is ... [Pg.50]

The supporting electrolyte may be 0.5 M potassium nitrate for bromide and iodide for chloride, 0.5 M potassium nitrate in 25-50 per cent ethanol must be used because of the appreciable solubility of silver chloride in water. [Pg.544]

Precipitated silver chloride dissolves in ammonia solutions as a result of the formation of Ag(NH3)2+. What is the solubility of silver chloride in 1.0 M NH.(aq) ... [Pg.601]

For example, adding silver nitrate solution to test for Cl (aq) is effective due to the very low solubility of silver chloride. You can use the precipitation of an insoluble salt to remove almost all of a particular ion from a solution and, as a result, cause a shift in the position of equilibrium of the original solution. The common ion effect is important in the solubility of salts. The precipitation of insoluble salts is used to identify the presence of unknown ions. You will learn more about the common ion effect in Chapter 9. [Pg.363]

To illustrate your answer, calculate and compare the molar solubility of silver chloride, AgCl (Kgp = 1.8 x 10 ), with silver chromate,... [Pg.442]

Consider the case in which the solubility of silver chloride is being measured by using a silver ion-selective electrode (ISE). The ISE is immersed in a solution... [Pg.103]

Table 19.6 lists Popoff and Neuman s values [3] of the solubility of silver chloride (AgCl) in water containing solvent electrolytes at the concentrations indicated. According to the same authors, the solubility of silver chloride in pure water is 1.278... [Pg.467]

TABLE 19.6. Values of the Solubility of Silver Chloride in Water Containing Solvent Electrolytes at the Concentration Indicated [3]... [Pg.467]

Commercial ISEs are widely available for various ions. Usually the ion-selective layer is made from an insoluble salt of the ion in question. For example, a chloride-detecting electrode can be made where the selective layer is a pellet of AgCl. Because of the very low solubility of silver chloride, the pellet never reaches equilibrium with the solution. Instead a small amount of chloride dissolves in the sample, leaving a relative surplus of silver atoms at the pellet... [Pg.100]

The solubility of silver chloride in water is about 10-5 M at 25°C, which sets a lower limit on the use of the electrode as an ion-specific electrode for chloride ion. The solubility in saturated KC1 solution increases to about 6 X 10-3 M, due to the formation of soluble complexes of the type AgCl. For this reason the saturated KC1 electrolyte must be presaturated with silver chloride otherwise the electrode becomes stripped of its AgCl coating. [Pg.189]

Physical Condition of the Solid Phase.—As long ago as 1870 Stas observed that the solubility of silver chloride varies with its method of preparation,4 the following results being obtained ... [Pg.314]

The exchange of silver ion between a precipitate of silver chloride and a solution of silver nitrate reaches isotopic equilibrium very rapidly (152). Because of the low solubility of silver chloride, a favorable ratio exists at equilibrium between the silver atoms in the precipitate and in the solution. For this reason, If a silver chloride precipitate is added to a solution containing only- trace amounts of radioactive silver, a high percentage of this radioactive silver will have exchanged with the silver in the precipitate by the time equilibrium is attained. [Pg.44]

Table 1.13 The effect of sodium chloride on the solubility of silver chloride...

The separation is based upon the solubility of silver chloride in dilute ammonia solution and the practical insolubility of silver iodide in this reagent. [Pg.386]

In Stas s second research allowance was made for the solubility of silver chloride in water, and for the presence of a trace of silica in the salt. Clarke has calculated the weighted mean of these four series of experiments to be... [Pg.89]

The standard potential of the silver azide electrode, i.e., Ag AgN3(s) N3", is -0.2919 V at 25°C. If the solubility of silver chloride is 1.314xl0 5 molal, calculate that of silver azide at 25°C. (Complete dissociation may be assumed for the dissolved material in the saturated solution in each case.)... [Pg.443]

For a uni-univalent salt the saturation solubility in pure water is thus equal to the square-root of its solubility product alternatively, it may be stated that the solubility product is equal to the square of the solubility in water. The solubility of silver chloride in water at 25 is 1.30 X 10 mole per liter the solubility product is consequently 1.69 X 10 . [Pg.171]

The concentration c of the silver salt in the ammonia solution may be regarded as consisting entirely of the complex ion, since the normal solubility of silver chloride is very small, so that Cx is virtually equal to c the concentration of the chloride ion may be taken as me because of the reaction... [Pg.174]

In order to derive m it is necessary to determine the solubility of silver chloride in ammonia in the presence of an excess of chloride ions equation (119) then takes the form... [Pg.174]

The value derived from the solubility of silver chloride obtained by the conductance method is 1.71 X 10 i . [Pg.255]

Ldalide Complexes. Silver halides form soluble complex ions, AgX J and AgX , with excess chloride, bromide, and iodide. The relative stability of these complexes is 1 > Br > Cl. Complex formation affects solubility gready. The solubility of silver chloride in 1 AIHCl is 100 times greater than in pure water. [Pg.90]

If a succession of complexes is formed, a corresponding number of terms from (7-34) must be added. For example, Forbes and Cole expressed the solubility of silver chloride by... [Pg.135]

EXAMPLE 7-8 From the above equilibrium constants, estimate the solubility of silver chloride in solutions containing chloride at the following concentrations 10 , 10 , 10 1, and 2 M. What is the minimum solubility, and at what chloride ion concentration does it occur ... [Pg.135]

Figure 7-2 represents data for solubility of silver chloride plotted to illustrate the minimum solubility, the common ion effect and intrinsic solubility S°, and the formation of the chloro complex. As Figure 7-25 indicates, at low concentrations of excess chloride an essentially linear relation is obtained between solubility and the reciprocal of the product of chloride ion concentration and the square of the activity coefficient. The zero intercept corresponds to S° (in this case an intrinsic solubility... [Pg.135]

For example we may consider the solubility of silver chloride in aqueous nitric acid solutions at 25 °C and at atmospheric pressure. We assume that AgCl dissociates practically completely in solution, in accordance with the reaction... [Pg.442]

Fig. 27.1. Solubility of silver chloride in the presence of nitric acid.

It is found experimentally that the solubility is related in a simple way to the ionic strength at sufficiently low ionic strengths the logarithm of the solubility of silver chloride varies linearly with the square root of I as illustrated by the experimental data in fig. 27.1. has the equation... [Pg.443]

The solubility of silver chloride in pure water is 1.314 X 10 molal, and the mean ionic activity coefficient is then 0.9985 [Neuman, J. Am. Chem. Soc., 54, 2195 (1932)]. The heat of solution of the salt is 15,740 cal. mole". Taking the entropy of solid silver chloride as 22.97 e.u. mole ", and using the results of the preceding exercise, calculate the standard free energy and heat of formation and the entropy of the Cl" ion at 25 C. [Pg.498]

So far, we have learned that if we know the chemical equilibria involved in a system, we can write a corresponding system of equations that allows us to solve for the concentrations of all species in the system. Although the systematic method gives us the means to solve equilibrium problems of great complexity, it is sometimes tedious and time consuming, particularly when a system must be solved for various sets of experimental conditions. For example, if we wish to find the solubility of silver chloride as a function of the concentration of added chloride, the system of five equations and five unknowns must be solved repetitively for each different concentration of chloride (see Example 11-9). [Pg.287]

As shown by Example 11-8, both Reaction 11-23 and Reaction 11-24 contribute to the solubility of silver chloride in water. [Pg.295]

The solid curve in Figure 11 -2 illustrates the effect of chloride ion concentration on the solubility of silver chloride data for the curve were obtained by substituting various chloride concentrations into Equation 11-41. Note that at high concentrations of the common ion, the solubility becomes greater than that in pure water. The broken lines represent the equilibrium concentrations of the various silver-containing species as a function of Ckci- Note that at the solubility minimum, undissociated silver chloride, AgCl(ag), is the major silver species in the solution, representing about 80% of the total dissolved silver. Its concentration is invariant, as has been demonstrated. [Pg.299]

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