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Study the effects of temperature on solubility of a salt.

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Introduction

Chemistry lab report Aim-to study the effects of temperature on solubility on a salt. Hypothesis-if the temperature is increased then the solubility of a salt should increase. This is because as the temperature rises the ionic bonds slightly weaken and thus the ions can take up the space between molecules of water. Even as the temperature increases the kinetic energy of the molecules increase, causing the molecules and ions to move faster and take up the space in between. Thus solubility increases. Variables-1.dependant variables-the solubility of the salt 2.independent variables-the temperature of the solution 3.controlled variables-1.the pressure applied 2.the nature of liquid (distilled water) 3.the presence of other ions. Apparatus-1.3 beakers 2.a stirring rod 3.filter papers 4.funnel 5.Bunsen burner 6.tripod stand 7.sodium chloride 8.potassium nitrate 9.zinc sulphate 10.spatula 11.flasks 12.distilled water 13.digital balance Method- 1.take 40 ml of distilled water in the beaker at room temperature and weigh it. ...read more.

Middle

Mass of the beaker+water (+/-0.01gm)- Mass of salt dissolved=mass of beaker+salt solution-mass of beaker+water Name of the salt Mass of salt dissolved at room temp. (+/-0.01gm) Mass of salt dissolved at 50degree Celsius. (+/-0.01gm) Mass of salt dissolved at 80 degree Celsius. . (+/-0.01gm) Sodium chloride Potassium nitrate Zinc sulphate Name of salt Volume of water taken (0.1ml) Mass salt dissolved. (0.02gm) Solubility (g/ml) Sodium chloride Potassium chloride Zinc sulphate Conclusion and evaluation-while conducting the experiment it was realized that the following problems were faced-1.the main problem that faced was to keep the temperature constant at 50 and 80 degree Celsius. Also this would cause a problem while the solutions are filtered because as the solution would filter the temperature of the solution would decrease and the dissolved salt would crystallize out and the result would not be obtained. ...read more.

Conclusion

If the temperature has fallen then the solution can be re heated without much hassle. Also, since it is not sensible to filter the solutions not at room temperature, excess of salt should be added so that the undissolved salt remains at the bottom and solution can just be transferred to another beaker. A problem encountered with this method is that some solution may remain behind and also that some undissolved salt may be accidentally transferred. But anyhow the variations are lesser than when the solution is filtered. As is seen in the observation table the solubility of a salt increases with increase in temperature. This is because as the kinetic energy of the solute as solvent molecules increase the bonds between ions of the salt and the forces between solute molecules weakens the solute ions easily fit in between molecules thus the solubility increases. ...read more.

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