It was found that the molar solubility of baso3 in 01 m is 80 x 10-6 m what is the value of ksp baso3?

Answer 1

here is your answer solubility = [Ba2+]= 80 x 10-6 M When BaSO3 dissolves it gives equal concentration of Ba2+ and SO32-, so Ksp = [Ba2+][SO32-] = 6.4 x10-9

Molar solubility is the number of moles of a substance (the solute) that can be dissolved in one liter of solution before the solution becomes saturated. It can be calculated from a substance's Solubility Product constant (Ksp) and the number of moles which dissociate in solution. The units are mol/L or M.

Molar Solubilities and Solubility Products
Solubility products, Ksp, of salts are indirect indication of their solubilities expressed in mol/L (called molar solubility). However, the solubility products are more useful than molar solubility. The molar solubilities are affected when there are common ions present in the solution. We need to employ the solubility products to estimate the molar solubilities in these cases.

When a salt is dissolved in pure water, solubility products and molar solubilities are related. This is illustrated using calcium carbonate. If x is the concentration of Ca2+ (= [CO32-]) in the saturated solution, then
Ksp = x2
In this case, x is also called the molar solubility of CaCO3. The following examples illustrate the relationship between solubility products, Ksp, and molar solubilities.

Examples 1
The Ksp for AgCl is 1.8e-10 M2. What is the molar solubility of AgCl in pure water?

Solution
Let x be the molar solubility, then

     AgCl  =  Ag+  +  Cl-
              x       x

     x = (1.8e-10 M2)1/2
       = 1.3e-5 M

Discussion

The solubility product, Ksp is a better indicator than the usual solubility specification of g per 100 mL of solvent or moles per unit volume of solvent.

For the AgCl case, when the cation concentration is not the same as the anion concentration ([Ag+] =/= [Cl-]) solubility of AgCl can not be defined in terms of moles per L. In this case, the system can be divided into three zones. The condition [Ag+] [Cl-] = Ksp, is represented by a line which divides the plane into two zones.

When [Ag+] [Cl-] < Ksp, no precipitate will be formed.

When [Ag+] [Cl-] > Ksp, a precipitate will be formed.

When AgCl and NaCl dissolve in a solution, both salts give Cl- ions. The effect of [Cl-] on the solubility of AgCl is called the Common ion effect