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 the common ion effect: Trial 1: Final Buret reading (ml)-29.50; Initial Buret reading (ml)- 26.10; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-33.30; Initial Buret reading (ml)- 29.50; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 3.40ml; Trial 2- 3.80mL. Report in proper sigfigs. 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. Use the dilution formula to determine the initial concentration of the common ion. C1V1 = C2V2 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. Make sure to include the effect of the common ion in the calculation.
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 the common ion effect:
Trial 1: Final Buret reading (ml)-29.50; Initial Buret reading (ml)- 26.10; Temperature (Celcius)- 25
Trial 2: Final Buret reading (ml)-33.30; Initial Buret reading (ml)- 29.50; Temperature (Celcius)- 25
Voume of HCl used: Trial 1- 3.40ml; Trial 2- 3.80mL. Report in proper sigfigs.
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. Use the dilution formula to determine the initial concentration of the common ion.
C1V1 = C2V2
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. Make sure to include the effect of the common ion in the calculation.
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