While transferring the weighed salt to the test tube in this experiment a studen
ID: 509929 • Letter: W
Question
While transferring the weighed salt to the test tube in this experiment a student accidently spilled some of their sample. How will this salt loss affect the salt solubilities calculated by this student? Will they be high, too low, or unaffected? Explain. It is important to keep the test tube closed to avoid evaporation of water while heating the salt solution. Briefly explain how a loss of water by evaporation would affect the initial calculation of the solubility of your salt. How would this affect your calculated value of K_sp? Assuming that the loss of water evaporation affected all subsequent calculated by the values of concentrations in the same manner, how would this ultimately affect delta H and delta S obtained by graphical analysis. Explain the chemical significance of the entropy change for dissolution of a salt.Explanation / Answer
Post lab
1) If some of salt is accidentally spilled by the student, the solubility found would be too high as now less amount of total salt is in solution and thus the amount of salt actually present to the salt dissolved would be higher than theoretical value.
2) It is important to avoid evaporation
a) Loss of water would change the weight of salt in solution and thus the initial amunt taken would be lower than the actual amount which would increase the solubilioty of salt in solution.
b) The calculate Ksp would thus be greater than the expected value,
c) dH would be greater for lower amount of salt in solution and dS would be higher.
3. Entropy of the salt in solution goes up or increases as it dissolved as more number of free ions are formed which increase the randomness of the systems. Thus a salt wih higher Ksp would also have higher entropy of solution.
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