Thank you for registering.

One of our academic counsellors will contact you within 1 working day.

Please check your email for login details.
MY CART (5)

Use Coupon: CART20 and get 20% off on all online Study Material

ITEM
DETAILS
MRP
DISCOUNT
FINAL PRICE
Total Price: Rs.

There are no items in this cart.
Continue Shopping

Why CsCl has got more solubility than NaCl though hydration enthalpy of Na is more??????

Why CsCl has got more solubility than NaCl though hydration enthalpy of Na is more??????

Grade:12

1 Answers

Arun
25763 Points
2 years ago
Dear student
 
I think you are wrong here as CsCl has less solubility than NaCl.

The solubility of the chlorides decreases as the group descends as the exothermic hydration enthalpy of the ions decreases at a greater rate than the endothermic lattice enthalpy of the ionic compound. This is because the Cl- ion is larger than a molecule of H20 meaning that the decrease in lattice enthalpy (due to the increase in atomic radius of the positive ion as you go down the group) is more significant than the decrease in hydration enthalpy of the cation (the hydration enthalpy of Cl- remains constant). Therefore the overall process becomes more endothermicand solubility decreases down the group as the reaction is less energetically favourable and less likely to go to completion (the ionic solid will exist in dynamic equilibrium with its ions in solution).

Therefore, CsCl is the least soluble of these group 1 chlorides, and NaCl is the most soluble.


 
 

Think You Can Provide A Better Answer ?

Provide a better Answer & Earn Cool Goodies See our forum point policy

ASK QUESTION

Get your questions answered by the expert for free