2. it is important to keep the test tube closed to avoid evaporation of water wh

Question

2. it is important to keep the test tube closed to avoid evaporation of water while heating the salt solution.

a) Briefly explain how a loss of water by evaporation would affect the inital calculations of the solubility of your salt.

b) How would this afect your calculated value of Ksp?

c) Assuming that the loss of water bt evaporation affected all subsequent calculated concentrations in the same manner, how would this ultimately affect the valuues of delta H and delta S obtained by graphigal anaylsis

3) Explain the chemical significance of entrophy change for dissolution of a salt

ab Questions hile transferring the weighed experiment, student cidently spilled some of their sample. How lculated by ailekled? Expl student? Will then be high too lowor is impoetanu lokeep hetest tubeclosed toawoxievaporation of water while heating a. Briefly expl how a loss of water by evaporation would affect the initial thesolubility of wor b. Hem would this ad your calculated value of k, Assuming that the loss of Mater by affect bsequent the AH and AS obtainer Explainthe chemical gnifianoe of the entropy change lordi

Explanation / Answer

a) If some water gets evaporated from the solution then it means that if we have started with saturated solution then it will decrease the solubility of salt and salt will appear undissolved in the solution (ppt of solute)

b) Ksp is calclated by calculating the mass of solute dissolved in the solution , it will decrease the solubility of salt and hence Ksp will also decrease

c) DeltaH and Delta S are calculated from graph by plotting 1/T v/s lnKsp

lnKsp will change, (decrease)

DeltaH = -slope X R

Delta S = intercept X R

so both will decrease

3) We know that

DeltaG = DeltaH - T deltaS

For a spontaneous process Delta G < 0

For this Delta S should be high (positive) as Delta H is positive

dissolution of solute should increase in entropy of solution.

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