wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

The solubility of Ba(OH)2.8H2O in water at 288 K is 5.6g per 100 g of water. What is morality of hydroxide ions in saturated solution of barium hydroxide at 288 K?(atomic masses:Ba - 137,O-16,H-1)

Open in App
Solution

The molecular mass of Ba(OH)2 = 315.4639 g/mol
Given that,
5.6g in 100g of water, which is the same as 56 g in 1kg of water.
Therefore, the number of moles of Ba(OH)2 in 1kg of water =56315.4639 = 0.1775 moles
The dissociation of Ba(OH)2 is as follows.


Ba(OH)2.8H2OBa2+(aq)+OH+(aq)+8H2O(l)


As specified in the balanced equation,
1 mol of Ba(OH)2 produces 2 moles of OH- ions.
Hence, No of moles of OH- ions = 2×0.177=0.355molesAs molality is moles of solute per kilogram of solvent,

Molality of OH- ions = 0.355 moles


flag
Suggest Corrections
thumbs-up
22
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Potassium Hydroxide
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon