Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used) moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction. 3. Calculate the molar solubility (in mol/L) of OH- and Ca2+. 4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)2 6. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature value. (Ksp of Ca(OH)2 = 8.0 × 10-6 at 25°C)
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask
Titration data for the determination of solubility and Ksp of calcium hydroxide:
Trial 1: Final Buret reading (ml)-19.80; Initial Buret reading (ml)- 13.00; Temperature (Celcius)- 25
Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25
Voume of HCl used: Trial 1- 6.80ml; Trial 2- 6.30mL
1. Compute for the moles of H+ used and the moles of OH- present.
moles of H+ used = (concentration of HCl) × (volume of HCl used)
moles of OH- = moles of H+ used
2. Construct an ICE table for the reaction.
3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.
4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)2
6. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature value.
(Ksp of Ca(OH)2 = 8.0 × 10-6 at 25°C)
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