Define the solubility product constant expression, Kop, for the dissolution of a
ID: 502505 • Letter: D
Question
Define the solubility product constant expression, Kop, for the dissolution of a sparingly soluble salt List as many experimental techniques as you can that may be used to determine the K_p for a sparingly soluble salt Suppose you place 1.0 g of Cu(IO_3) 2 in contact with 50 mL of distilled water and gently stir the mixture. Sketch a graph in your laboratory notebook showing how the concentrations of Cu^2+ and IO_3^-, in solution will change with time, assuming that solid and liquid are placed in contact at t=0. The plot should be qualitative. Describe what happens at the molecular level once equilibrium is reached--that is, once the solution is saturated with Cu(IO_3)_2. Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibrium? Describe how you are going to calculate the [Cu^2+] for the saturated solution of copper iodate once you know the absorbance value of the copper ion How will you use this concentration to find the K_ep value for copper iodate? A student performed the lodate Analysis and found that it took 7.80 mL of 0.02 M Na_2S_2O_3 to titrate 4.00 mL of saturated copper iodate. Answer the following questions: Using the balanced equations on page 79, what is the mole ratio of triiodide, I_3^-, to thiosulfate, S_2O_3^2-? What is the mole ratio of iodate, IO_3^- to triiodide, I_3? Calculate the number of moles of iodate in 7.80 mL of 0.02 M Na_2S_2O_3. What is the iodate concentration in the 4.00 mL of saturated copper iodate solution? Use this value to find the K_ep Value for copper iodate? AgCl is placed in contact with 100.0 mL of distilled water. Given the K_sp for Agcl is 1.8 times 10^-10, answer the following questions: Write the equation representing solid silver chloride in equilibrium with its ions, Ag^+ and Cl^- What is the K_sp expression for this equation? From the K_sp expression, calculate [Ag^+]and [Cl^-] What mass of AgCl will dissolve in the 100.0 mL of water?Explanation / Answer
Answer (1)
Solubility Product Constant Expression
Solubility is the ability of a substance to dissolve in water. The solubility is measured in terms of concentration of an ion that is present in a smaller ratio in solution. On the other
hand, solubility equilibrium refers to the equilibrium between the dissolved salt (ions) and undissolved salt that usually exists in a saturated solution or a solution of a sparingly
soluble salt. The word sparingly soluble salt refers to a salt that is partially (not completely) soluble in water, as results of which, the equilibrium between dissolved ions and undissolved salt is possible.
AgCl(s) <------> Ag+(aq) + cl-(aq)
Since this is an equilibrium reaction, we can write the equilibrium constant expression as
K = {(Ag+) (Cl-) } / { AgCl (s) }
The concentrations of solids are either unknown or assumed to be constant. Hence we combine [AgCl(s)] with K and label this constant as Ksp. Thus
Kx [AgCl(s)] = Ksp = [Ag+] [Cl-]
The Ksp is called the solubility product constant or simply solubility product.
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