Ionic EquilibriumHard
Question
A solution prepared by dissolving 2.8 g of lime (CaO) in enough water to make 1.00 L of lime water (Ca(OH)2(aq.)). If solubility of Ca(OH)2 in water is 1.48 gm/lt. The pH of the solution obtained will be:
[log 2 = 0.3, Ca = 40 , O = 16, H = 1]
[log 2 = 0.3, Ca = 40 , O = 16, H = 1]
Options
A.12.3
B.12.6
C.1.3
D.13
Solution
Ca(OH)2 ⇋ Ca2+ + 2OH-
t = 0
= 0.02 0 0
teq 0 0.02 0.04
so, pOH = 2 - log 4 = 1.4
so pH = 12.6
t = 0
= 0.02 0 0teq 0 0.02 0.04
so, pOH = 2 - log 4 = 1.4
so pH = 12.6
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
What is the minimum pH when Fe(OH)3 starts precipitating from a solution containing 0.1M FeCl3? Ksp of Fe(OH)3 = 8 ×...In which of the following acid-base titration, pH is greater than 8 at equivalencepoint....What concentration of free CN– must be maintained in a solution that is 1.8 M-AgNO3 and 0.16 M-NaCl to prevent AgCl from...The solubility product of Zn(OH)2 is 10–14 at 25oC. What would be the concentration Zn+2 ion in 0.1 M-NH4OH solution whi...Complete hydrolysis of cellulose gives...