Investigating the Solubility of 5 Salts

1. PurposeThe trys were carried out for measurement of solvability of 4 elect salts in water to arrange these salts in the ascending stage of solubility.2. IntroductionDifferent salts raise in water to different extent. This fact is of great importance in our daily life as well as in industrial domain like extraction of useful mineral/metal, purification of salts, eroding etc. Solubility of salts is quantitatively expressed in different units. The close to common being maximum bus of a salt which can be completely dissolved in a unit mass of a solvent say 14 gm of KNO3 per c gm of water i.e. of gm solute/gm solvent type. Other units atomic number 18 yard (M), Molality (m), Normality (N), Mole fraction (X) etc. These different units are useful in different situations. It is easiest to experiment eachy restrict the solubility of a salt in gm (of salt)/ nose candy gm (of solvent) unit and this appreciate can easily be converted into other units by exploitation suitable fo rmulae. The formula to convert gm solute/gm solvent solubility value into molarity (M) is followingM = (1)Where, is density of solution in g/liter and formula mass is in g/mol.Materials are classified as insoluble, slightly soluble or soluble. Materials with solubility little than 0.01M are classified as insoluble.Experiments were carried out to measure solubility of quad salts Calcium sulphate CaSO4, Copper (II) Nit browse Cu(NO3)2, Potassium Nitrate KNO3 and atomic number 11 Chloride NaCl.3. MaterialsApproximately five grams of each of salts Ammonium Nitrate NH4NO3, Calcium Sulfate CaSO4, Copper (II) Nitrate Cu(NO3)2, Potassium Nitrate KNO3 and Sodium Chloride NaCl, 250 ml beaker, 100 ml beaker, 50 ml burette and Parr DMA 35 density meter.4. mental process4.1. Ammonium Nitrate NH4NO3 salt was ground into fine powders using a mortar and pestle.4.2. Approximately 5 gm of the salts was weighed using a dimension and the exact mass was record for each of the salts.4.3. The sal t powder was set in a clean 250 ml beaker.4.4. Water was added slowly using 50 ml burette and the solution was continuously stirred speckle water was being added. Water addition was done until either all the salt powder was dissolved or 50 ml was reached, whichever occurred first.4.5. rule book of water required for complete dissolution of the salt powder was recorded.4.6. immersion and temperature of the saturated salt solution was measured by using Parr meanness meter and the same was recorded.4.7. Steps 4.1 through 4.6. were repeated for the remaining intravenous feeding salts and the values were recorded in a table.5. DataThe data from this experiment is presented in table 1 belowTable 1 observational data on solubility of the saltsSalt Mass of Salt (gm) Volume of water system (ml) Temperature (oC) Density of Solution (gm/ml) CaSO4 5.088 50 none None Cu(NO3)2 5.020 23 30.4 1.125 KNO3 4.956 48 16.9 1.065 NaCl 4.993 49 20.2 1.0656. Results and AnalysisFrom data it is very c lear that CaSO4 is insoluble in water.Solubility of remaining three salts was calculated using formula 1.For Cu(NO3)2M = 1.07 at 30.4 oC wherefore solubleFor KNO3M = 1.00 at 16.9 oC Hence solubleFor NaClM = 1.20 at 20.2 oC Hence solubleThe results are presented in table 2 in the ascending order of solubility.Table 2 Solubility of given saltsSalt Solubility of Salt (g/100 g of water) Solubility of Salt (M) Temperature (oC) CaSO4 0 Insoluble Not recorded KNO3 10.35 1.00 16.9 Cu(NO3)2 21.83 1.07 30.4 NaCl 10.20 1.20 20.2 The order of solubility of salts is followingCaSO4 KNO3 Cu(NO3)2 NaClThis order may get slightly limited if we compare solubility of salts at same temperature. It should be noted that solubility value depends on temperature and this is the reason, why solubility value is reported along with temperature.Glassware has been used in these experiments at visibility of solution was required to determine that salts were completely dissolved. Besides, these glass wares provid e reasonable accuracy and are sanely less costly.The salts were ground into fine powder because fine powders accelerate rate of dissolution of salts, hence the experiment can be finished in short span of time.