1. Using the titration data, determine the concentration of hydroxide ion in the saturated Ca(OH)2 in Titration #1. Data

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1. Using the titration data, determine the concentration ofhydroxide ion in the saturated Ca(OH)2 in Titration #1.
Data Table
Titration #1
Saturated Ca(OH)2
Titration #2
Saturated Ca(OH)2 prepared in CaCl2 (aq)
Volume Ca(OH)2 (mL)
25 mL
25 mL
pH of Ca(OH)2
12.11
11.96
HCl Concentration (M)
0.1081M
0.1081M
Initial Buret Reading (mL)
0.00 mL
0.00 mL
Final Buret Reading (mL)
10.40 mL
8.64 mL
Volume HCl delivered (mL)
10.40 mL
8.64 mL
2.Determine the concentration of calcium ion in Titration#1.
3.What is the molar solubility of Ca(OH)2 in the saturatedsolution?
4.Determine the Ksp for Ca(OH)2
5.Using the titration data, determine the concentration ofhydroxide ion in the saturated Ca(OH)2 containing the common ion inTitration #2.
6.Determine the concentration of calcium ion (from the Ca(OH)2only) in Titration #2.
7.What is the molar solubility of Ca(OH)2 in the saturatedsolution prepared in CaCl2 (aq)?
8.Look up the Ksp for Ca(OH)2 in your textbook and calculate thepercent error in this experiment.
9.Once again, calculate the concentration of hydroxide ion inthe saturated solution (in the Titration #1 column), but this timeutilize the pH to determine the hydroxide ionconcentration.
10.Once again, calculate the calcium ion concentration in thesolution based on your answer in 9 above, then determine the Kspfor Ca(OH)2.
11.Determine the percent error for the Ksp value obtained innumber 10 above.
12.Compare the percent error from problems 8 and 11. Suggest reasons why the different experimental data provide suchdifferent results. (Think about the sources for experimentalerror with each method.)