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Solubility Product Determination Lab

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Solubility Product Determination Lab
Solubility Product Determination

Purpose • To determine the solubility product constant, Ksp, of an ionic compound.

Introduction The solubility product constant, Ksp, is a particular type of equilibrium constant. The equilibrium is formed when an ionic solid dissolves in water to form a saturated solution. The equilibrium exists between the aqueous ions and the undissolved solid. A saturated solution contains the maximum concentration of ions of the substance that can dissolve at the solution’s temperature. The equilibrium equation showing the ionic solid lead chloride dissolving in water is:

PbCl2(s) ( Pb2+(aq) + 2Cl-(aq)

The solubility product expression is:

Ksp = [Pb2+][Cl-]2

A knowledge of the Ksp …show more content…
Place 5 drops of 0.10 M sodium hydroxide in each of the wells #1 through #12. Stir thoroughly with a toothpick. 7. Allow three or four minutes for the precipitates to form. Observe the pattern of precipitation. Record.

Part II Ksp by dilution of hydroxide ions. 1. Repeat the procedure in Part I, but use a serial dilution of NaOH followed by 5 drops of calcium nitrate in each well.

Data Analysis

Part I 1. Determine the concentration of the calcium ion in each well after the serial dilution but before the sodium hydroxide has been added. 2. Determine the concentration of the calcium ion in each well after the sodium hydroxide has been added. 3. Determine the concentration of the hydroxide ion in each well. 4. Assume that the first well with no precipitate contains a saturated solution. Calculate the solubility product of calcium hydroxide using the concentrations in this well.

Part II 1. Determine the concentration of the hydroxide ion in each well after the serial dilution but before the calcium nitrate has been added. 2. Determine the concentration of the hydroxide ion in each well after the calcium nitrate has been added. 3. Determine the concentration of the calcium ion in each …show more content…
Again calculate the solubility product of calcium hydroxide using the concentrations in the first well that has no precipitate. 4. Average the two values of Ksp determined in Parts I and II. 5. Look up the accepted value for the Ksp of calcium hydroxide and calculate percent error.

Data and Results

Part I

| Well # | [Ca2+] | [Ca2+] | [OH-] |Precipitate? |
| |before NaOH |after NaOH | | |

1
| | | | | |

2
| | | | |
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