How Do You Increase The Solubility Of An Ionic Compound In Water?
An ionic compound dissociates into ions (charged particles) in the solution. A classic example of ionic compounds is inorganic salts, such as sodium chloride (NaCl) or potassium nitrate (KNO3). The solubility characterizes how well a substance dissolves in solvent and is typically expressed in grams of the dissolved compound per 100 g of solvent. As a rule (with a few exceptions) the solubility of ionic compounds in water increases with temperature. To illustrate this principle, prepare the solution of potassium nitrate by dissolving 120 g of the salt in 200 ml of water. Divide the mass of the salt by the mass (volume) of water, and multiply the quotient by 100 to calculate solubility that is required to make the particular solution. In our example, it is (120 / 200) x 100 = 60 g/100 g water. Find solubility of the compound in question (see the Solubility Database link in Resources). In our example, the solubility of potassium nitrate is 31.6, 61.3 and 106 g /100 g water at temperature
