Solubility product expression

Substituting the equilibrium concentrations into the solubility product expression (equation 6.33)... [Pg.157]

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]

Write the solubility product expression for each of the following reactions. [Pg.178]

In reaction (7), all of the molecular species involved in the equilibrium are in the solution as dissolved species. Though the equilibrium relationship that exists among the concentrations is a little more complicated than in the solubility product expressions, the guiding principles are the same. [Pg.179]

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]

The solubility product principle states that the solubility product expression for a slightly soluble compound is the product of the concentrations of its constituent ions, each raised to the power that corresponds to the number of ions in one formula unit of the compound. The quantity, K, is constant at constant temperature for a saturated solution of the compound, when the system is at equilibrium. The significance of the solubility product is that it can be used to calculate the concentrations of the ions in solutions for such slightly soluble compounds. [Pg.337]

The ion product has the same format as the solubility product expression, but it involves initial rather than equilibrium concentrations. [Pg.459]

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]

Ion concentration terms in solubility product expressions are usually written without their phases, as you see here. [Pg.431]

Write the balanced chemical equation that represents the dissociation of each compound in water. Then write the corresponding solubility product expression. [Pg.432]

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

Step 2 Use the equation to write the solubility product expression. Step 3 Find the concentration (in mol/L) of each ion. [Pg.432]

How do you predict whether a given concentration of ions will result in the precipitation of an ionic compound How can you tell if a solution is saturated You substitute the concentrations of the ions into an expression that is identical to the solubility product expression. Because these concentrations may not be the same as the concentrations that the equilibrium system would have, however, the expression has a different name the ion product. [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]

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]

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]

A solution of barium chromate (BaCr04) is prepared by dissolving 6.3 X 10 g of this yellow solid in 1.00 L of hot water. Will solid barium chromate precipitate upon cooling to 25°C, 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]

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