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_sp 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.

Explanation / Answer

Q2.

experimental techniiques for Ksp determination:

In order to calculate Ksp, you need:

Concentration of ions, OR, solubilty of sample

so

First could be:

- Titration (acid/base) --> Zn(OH)2(s) --> Zn+2 + 2OH-

then

Use H+ to neutralize OH- ions, when pH indicator shift, you know you have your concentration

relate [OH-] with [H+]

then relate Zn+2 with OH-

finally

Ksp = [Zn+2][OH-]^2 can be calculated

- Via electropotential titration

Add electrictiy until species precipitate:

Cu3(PO4)2(s) <--> Cu+2(aq) + 2(PO4)(aq)

addition of electrons will:

Cu+2 + 2e- <--> Cu(s)

then, weight Cu, calculate moles, clacualte moalrity, relate molarity to

Ksp = [Cu+2]^2 * [PO4-3]^2

- Via gravimetry

Precipitate any specie of the salt such as:

AgI(s) <-- Ag+(aq) + I-(aq)

Precipitate Ag+ via AgBr

then calculate the mass of Ag+ present in the original sample

then

relate [Ag+] with AgI

then

Ksp = [Ag+][I-]

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