lOMoARcPSD|5967629
Reddy 1
lOMoARcPSD|5967629
Seminar Assignments, Experiment- Molar
Solubility, Common-ion Effect
General Chemistry II/Lab (Nova Southeastern
University)
Experiment 22: Molar Solubility, Common-Ion
Effect Niyanthesh Reddy
Lab Partners: Samir Nacer,
Kristen Date: 03/31/2016
Professor: Dr. Ballester
Lab Assistant: Dr. Sarah Rodriguez
, lOMoARcPSD|5967629
Reddy 2
Abstract
The purpose of this experiment was to understand the molar solubility and solubility constant
of Calcium Hydroxide, Ca(OH)2. Many principles were involved such as, Molar solubility is the
number of moles of salt that dissolves per liter of (aqueous solution), Solubility Product is the
equilibrium constant for a slightly soluble salt at Dynamic Equilibrium, and Common-Ion Effect
is the effect of an ion on the position of the equilibrium (Beran, 2013). In this experiment, a
Titration procedure was conducted, where 0.05 M concentrations of HCl was added to the
basic solution of Calcium Hydroxide to reach the stoichiometric point (indicated by methyl-
orange indicator). The molar solubility of Ca (OH) 2 in solution was 1.5 x 10-2 mol/L and the
average solubility product (Ksp) was 1.3 x 10-5 for Ca (OH) 2. Definitely the hypothesis of this study
was accepted, as first, Calcium Hydroxide being less soluble substance and HCl as being a
strongly titrating solution, so the solubility product would become less saturated, and as the
Common- Ion Effect did occur, so the molar solubility decreased and the equilibrium shifted
to the left (reactants).
Reddy 1
lOMoARcPSD|5967629
Seminar Assignments, Experiment- Molar
Solubility, Common-ion Effect
General Chemistry II/Lab (Nova Southeastern
University)
Experiment 22: Molar Solubility, Common-Ion
Effect Niyanthesh Reddy
Lab Partners: Samir Nacer,
Kristen Date: 03/31/2016
Professor: Dr. Ballester
Lab Assistant: Dr. Sarah Rodriguez
, lOMoARcPSD|5967629
Reddy 2
Abstract
The purpose of this experiment was to understand the molar solubility and solubility constant
of Calcium Hydroxide, Ca(OH)2. Many principles were involved such as, Molar solubility is the
number of moles of salt that dissolves per liter of (aqueous solution), Solubility Product is the
equilibrium constant for a slightly soluble salt at Dynamic Equilibrium, and Common-Ion Effect
is the effect of an ion on the position of the equilibrium (Beran, 2013). In this experiment, a
Titration procedure was conducted, where 0.05 M concentrations of HCl was added to the
basic solution of Calcium Hydroxide to reach the stoichiometric point (indicated by methyl-
orange indicator). The molar solubility of Ca (OH) 2 in solution was 1.5 x 10-2 mol/L and the
average solubility product (Ksp) was 1.3 x 10-5 for Ca (OH) 2. Definitely the hypothesis of this study
was accepted, as first, Calcium Hydroxide being less soluble substance and HCl as being a
strongly titrating solution, so the solubility product would become less saturated, and as the
Common- Ion Effect did occur, so the molar solubility decreased and the equilibrium shifted
to the left (reactants).
