the hydrated salt Na2SO4. 10H2O undergoes X%loss in weight on heating and become anhydrous. the value of X will be
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Answered by
41
Given reaction: Na2SO4.10H2O——>Na2SO4 + 10H2O
Here moles of Na2SO4.10H2O = 1 mole
Because, weight of substance = no. of moles* molecular weight
Therefore, weight of substance = 1*(46+32+64+180)
= 322g
Similarly, weight of anhydrous Na2SO4 = 180g
Therefore, percentage loss = [(320-180)/322]*100
=55.90%
Here moles of Na2SO4.10H2O = 1 mole
Because, weight of substance = no. of moles* molecular weight
Therefore, weight of substance = 1*(46+32+64+180)
= 322g
Similarly, weight of anhydrous Na2SO4 = 180g
Therefore, percentage loss = [(320-180)/322]*100
=55.90%
Answered by
1
Answer:
56%
Explanation:
molecular mass of Na2So4=322
on heating the Na2So410H2o it becomes anhydrous that means 10H2o molecules seprated
molecular mass of10H2o =180
%loss = 180/322×100=55.9%=56%
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