Define the solubility product constant expression, K_sp, for the dissolution of

Question

Define the solubility product constant expression, K_sp, 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): 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. 4. 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 u 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_sp value for copper iodate? A student performed the Iodate 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, IV, 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_sp 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^+J and [Cl^-]. What mass of AgCl will dissolve in the 100.0 mL of water?

Explanation / Answer

Q1.

Define Ksp, for a sparingly soluble salt:

Note that not all salts will be soluble at given T, solvent

for water, there is a limit for each salt amount which will be in solution

Typically, for a salt "AB":

AB(s) <--> A+(aq) + B-(aq)

the equilibrium

K = [A+][B-]/[AB]

since AB is solid, then

K*[AB] = Ksp = [A+][B-]

This is the quotient for this speicifc satl, AB

but for more complex salts such as

A3B2

expect

A3B2(s) <--> 3A+2(aq) + 2B-3(aq)

then

Ksp = [A+2]^3[B-3]^2

the Ksp will typically be much lower for these type of salts.

Therefore

Ksp is a rapid way to:

- Describe the solubility of a salt

- Relate ionic concentration of the salt

- Relate the overall solubility of Different salt

- Ksp is constant at a given T, will not vary unless T changes

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