Rinse and fill the buret with 0.100 M HCl solution. Transfer accurately 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) into two separate E-flasks. Add 2 drops of phenolphthalein to each flask and titrate each solution until the pink color disappears. Voume of HCl used: Trial 1= 6.80ml; Trial 2 = 6.30mL Determination of solubility and Ksp of calcium hydroxide 2. 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 3. Construct an ICE table for the reaction. 4. Calculate the molar solubility (in mol/L) of OH- and Ca2+. 5. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol) 6. Calculate the Ksp of Ca(OH)2. 7. 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)
Rinse and fill the buret with 0.100 M HCl solution. Transfer accurately 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) into two separate E-flasks. Add 2 drops of phenolphthalein to each flask and titrate each solution until the pink color disappears.
Voume of HCl used: Trial 1= 6.80ml; Trial 2 = 6.30mL
Determination of solubility and Ksp of calcium hydroxide
2. 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
3. Construct an ICE table for the reaction.
4. Calculate the molar solubility (in mol/L) of OH- and Ca2+.
5. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol)
6. Calculate the Ksp of Ca(OH)2.
7. 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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