Solubility Product Expression and

Consider a saturated solution of silver chloride that is in contact with undissolved solid silver chloride. The equilibrium can be represented as [Pg.701]

Although AgCl is not veiy soluble, all the AgCl that does dissolve in water dissociates completely into Ag and Cl ions. We can write the equilibrium expression for the dissociation of AgCl as [Pg.701]

Because each AgCl unit contains only one Ag and one CF ion, its solubility product expression is particularly simple to write. Many ionic compounds dissociate into more than two ions. Table 17.4 lists a number of slightly soluble ionic compounds along with equations representing their dissolution equilibria and their solubility product constants. (Compounds deemed soluble by the solubility rules in Chapter 4 are not listed for the same reason we did not list values for the strong acids in Table 16.6.) In general, the magnitude of indicates the solubility of an ionic compound—the smaller the value, the less soluble the compound. To make a direct [Pg.701]

There are two ways to express the solubility of a substance molar sohibiUty, which is the number of moles of solute in 1 L of a saturated solution (mol/L), and solubility, which is the number of grams of solute in 1 L of a saturated solution (g/L). Both of these expressions refer to concentrations of saturated solutions at a particular temperature (usually 25°Q. [Pg.701]

Often we know the value of Kgp for a compound and are asked to calculate the compound s molar solubility. The procedure for solving such a problem is essentially identical to the p ocedure for solving weak acid or weak base equilibrium problems [Pg.701]

Step 4 Substitute the concentrations into the solubility product expression, and calculate Ksp. [Pg.432]

TABLE 6.1 Solubility product expressions and fsp values for some minerals in the system Ca0-Mg0-C02 S03-H20 at 25 C and 1 bar total pressure... [Pg.194]

Solubility Equilibria Solubility Product Expression and Kgp Calculations Involving and Solubility Predicting Precipitation Reactions... [Pg.680]

Example A What is the solubility product expression and the molar solubility, S, of NiS (5), which has a ATsp of... [Pg.468]

At the equivalence point, we know that the concentrations of Agi" and CL are equal. Using the solubility product expression... [Pg.351]

Write the equation for the dissolving of calcium sulfate, CaSOt, and the solubility product expression. [Pg.174]

The relative molecular mass of magnesium hydroxide is 58.3. Each mole of magnesium hydroxide, when dissolved, yields 1 mole of magnesium ions and 2 moles of hydroxyl ions. If the solubility is xmolL-1, [Mg2 + ] = x and [OH-] = 2x. Substituting these values in the solubility product expression ... [Pg.26]

C18-0073. For the following salts, write a balanced equation showing the solubility equilibrium and write the solubility product expression for each (a) silver chloride (b) barium sulfate (c) iron(H) hydroxide and (d) calcium phosphate. [Pg.1339]

Electrodes responding to other halides, sulphide, cyanide, silver, lead, copper and cadmium are made using membranes fabricated from pure or doped silver sulphide (Ag2S). The membrane potential is affected by the movement of Ag+ ions between cationic lattice sites which in turn is determined by the activities of the Ag+ ion in the internal and sample solutions. As the activity of the former is fixed, that of the latter alone influences the membrane potential. The electrode will also respond to the presence of S2- ions because of their effect on the Ag+ ion activity via the solubility product expression ... [Pg.239]

Write a balanced dissolution equation and solubility product expression for silver carbonate, Ag2C03. [Pg.432]

The ion product, Qsp, is an expression that is identical to the solubility product constant, but its value is calculated using concentrations that are not necessarily those at equilibrium. (The relationship between the expression for solubility product, Kgp, and the expression for the ion product, Qsp, is analogous to the relationship between the equilibrium constant, iQ, and the reaction quotient, Qc.)... [Pg.443]

You can use the relationship between the ion product expression and the solubility product expression to predict whether a precipitate will form in a given system. One common system involves mixing solutions of two soluble ionic compounds, which react to form an ionic compound with a very low solubility. If Qsp > Kp. based on the initial concentrations of the ions in solution, the sparingly soluble compound will form a precipitate. [Pg.444]

Since the dissolution of a slightly soluble salt in water is an equilibrium, an equilibrium expression can be written. This expression is known as the solubility product. The constant for the expression is named the solubility product constant and denoted by K p. For example, the solubility product for the reaction below ... [Pg.88]

If we want to know how much Hgj1 is dissolved in a saturated solution of Hg2Cl2, we are tempted to look at Reaction 6-9 and to note that two Cl are created for each flg2. If we let x be the concentration of flg2, we could say that the concentration of Cl is 2 a. Substituting these values into the solubility product expression 6-10, we could write Ksp = [Hg2 fC1 2 = (a) (2a)2 and would find [ HgJf J = x = 6.7 X 10-7 M. [Pg.101]

Following the usual convention, we will now express all concentrations in moles per liter, and drop the units M2 from the solubility product expression. If solid silver chloride is added to water, dissociation of the solid will create an equal number of silver ions and chloride ions, hence the concentrations of silver ion and chloride ion will be the same. If we substitute x = [Ag+] = [Cl-] into Equation 1.2, this implies... [Pg.6]

Cubic and higher order polynomial expressions also arise naturally in a wide range of problems in chemistry, particularly in solubility and equilibrium problems. If we try to dissolve lead (II) chloride (PbCl2) instead of silver chloride, the solubility product expression becomes... [Pg.7]

Answer You still must start out by writing the solubility equilibrium and solubility product expression ... [Pg.355]

Chemistry is a very wide field however, only a very small portion, indeed, of this seemingly complex subject is used in this book. These include equivalents and equivalent mass, methods of expressing concentrations, activity and active concentration, equilibrium and solubility product constants, and acids and bases. This knowledge of chemistry will be used under the unit processes part of this book. [Pg.50]

Suppose a small amount of NaCl(s) is added to a saturated solution of AgCl. What happens Sodinm chloride is qnite solnble in water and dissolves to form Na (rjq) and Cl (aq) ions, raising the concentration of chloride ion. The quantity Qo = [Ag ][Cl ] then exceeds the K p of silver chloride, and silver chloride precipitates until the concentrations of Ag (aq) and Cl (aq) are snfficiently reduced that the solubility product expression once again is satisfied. [Pg.686]

Iron(III) sulfate, Fe2(S04)3, is a yellow compound that is used as a coagulant in water treatment. Write a balanced chemical equation and a solubility product expression for its dissolution in water. [Pg.700]

L of hot water and cooling the solution to 25°C. Will solid precipitate result from this process, according to the solubility product expression Explain. [Pg.701]

Write a chemical equation for the dissolution of mercury(I) chloride in water, and give its solubility product expression. [Pg.703]

The equilibrium of a solvation reaction has its own equilibrium constant called the solubility product Ksp. Use Ksp the same way you would use any other equilibrium constant. Remember that solids and pure liquids have an approximate mole fraction of one and can be excluded from the equilibrium expression. Thus, solids are left out of the solubility product expression as in the example of the Ksp for barium hydroxide shown below. [Pg.75]

It is of interest to determine how much iodide is precipitated before appreciable amounts of silver chloride form. With the appearance of the smallest amount of solid silver chloride, the solubility-product expressions for both precipitates apply, and division of one by the other provides the useful relationship... [Pg.356]

In some cases a compound contains more than two kinds of ions. Dissolution of the slightly soluble compound magnesium ammonium phosphate, MgNH PO, in water and its solubility product expression are represented as... [Pg.825]

In saturated solutions, equilibrium exists between soUd and dissolved solute. The equation for the dissolution of barium sulfate in water and its solubility product expression are... [Pg.826]

Solubility, Molar Solubility, and Solubility Product Expression... [Pg.827]

For part (a), we write the appropriate chemical equations and solubility product expression, designate the equilibrium concentrations, and then substitute into the solubility product expression. For part (b), we recognize that NaF is a soluble ionic compound that is completely dissociated into its ions. MgF2 is a slightly soluble compound. Both compounds produce F ions so this is a common ion effect problem. We write the appropriate chemical equations and solubility product expression, represent the equilibrium concentrations, and substitute into the solubility product expression. For part (c), we compare the molar solubilities by calculating their ratio. [Pg.830]

We start with the general solubility product expression /irsp[Al(OH)3] = [Al ][OH Given also that - [H ][OH ], we can eliminate OH" from the expre.ssion, and solve for [Al +] to... [Pg.248]

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