Determination of the solubility product of an ionic compound post lab answers
Answers
1 Data
The following data were collected. Dilution Precipitation well Ca2+ #6 OH− #4
2 Calculations
2.1 Calcium Ion Serial Dilution
The rst well without a precipitate is well number 6. The concentration of calcium ions per well is [Ca2+] = 0.10 2n M (1) where n is the well number. So, the concentration of calcium ions in well number 6 is 0.10 26 M = 1.6×10−3 M For each of the wells in this series, the concentration of added NaOH was a constant 0.1M 2 = 0.05M after being added to each well. The Ksp for this ion equilibrium, Ca(OH)2
Ca2+ +2OH−, is Ksp =Ca2+OH−2 (2) So, putting in the concentrations for well number 6, which is assumed to have complete dissociation of the calcium hydroxide, Ksp =1.6×10−3[0.05]2 = 3.9×10−6 1
2.2 Hydroxide Ion Serial Dilution
The rst well without precipitate for this series is well number 4. The concentration of hydroxide ions per well is [OH−] = 0.10 2n M (3) again, with n being the well number. So, the concentration of hydroxide ions in well number 4 is 0.10 24 M = 6.3×10−3 M Foreachofthewellsinthisseries, theconcentrationofaddedcalciumnitratewasaconstant 0.1M 2 = 0.05M after being added to each well. Using the ion equilibrium equation and these concentrations, we can nd that Ksp = [0.05]6.3×10−32 = 2.0×10−6 Then, ¯ Ksp = 3.9×10−6+2.0×10−6 2 = 3.0×10−6 The actual Ksp is 5.02×10−6 and the percent error from this value to the calculated average is |3.0×10−6−5.02×10−6|
Answer:
The determination of the solubility product of an ionic compound involves careful measurement and calculation, and it can provide valuable information about the properties of the compound and its behavior in solution.
Explanation:
As an AI language model, I do not have access to specific post-lab answers for any particular experiment. However, I can provide general information on how to determine the solubility product of an ionic compound based on the experiment.
The solubility product (Ksp) is a measure of the extent to which a sparingly soluble ionic compound dissolves in water, and it can be determined experimentally by measuring the concentration of the ions in the solution.
To determine the solubility product, you would typically perform the following steps:
Prepare a solution of the ionic compound at a known concentration.
Measure the concentration of one of the ions in the solution by using an appropriate analytical technique such as titration, spectrophotometry, or ion-selective electrode.
Use the stoichiometry of the balanced chemical equation for the dissolution of the compound to determine the concentration of the other ion.
Use the concentrations of both ions to calculate the solubility product of the compound using the following formula:
Ksp = [A+]^m [B-]^n
Where A+ and B- are the cations and anions of the compound, respectively, and m and n are their coefficients in the balanced chemical equation.
It is important to note that the solubility product is a constant at a given temperature and pressure, and it depends only on the nature of the compound and not on the amount of the compound present in the solution.
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