Question
THE SOLUBILITY PRODUCT CONSTANT FOR BaSO4 AT 298K IS 1.1X10-1O POWER. CALCULATE THE SOLUBILITY OF BaSO4 IN MOL\L AT 298K
Answers
Basically, when BaSO4 dissolves in water, it dissociates into the ions Ba^+2 and SO4^-2. The solubility product constant expression then becomes as follows:
Ksp=[Ba^+2][SO4^-2]
You already know that the Ksp for BaSO4 is 1.1x10^-10. This means that BaSO4, when it dissociates, has the same concentrstion for its ions.
Ksp=[Ba^+2][SO4^-2]
Ksp=[1.1×10^-10][1.1×10^-10]
Ksp=1.21×10^-20
Ksp=[Ba^+2][SO4^-2]
You already know that the Ksp for BaSO4 is 1.1x10^-10. This means that BaSO4, when it dissociates, has the same concentrstion for its ions.
Ksp=[Ba^+2][SO4^-2]
Ksp=[1.1×10^-10][1.1×10^-10]
Ksp=1.21×10^-20
Related Questions
Considering the effect of ionic strength, calculate the solubility of BaSO4 in 0.100 mol/L NaCl solu...
I have a question about solubility rules and net ionic equations
so for example :
CuSO4+Ba(NO3)...
Calculate the molar solubility of BaSO4 in a solution in which [H3O+] is 0.50 M. Ksp(BaSO4) = 1.1×10...
Calculate the molar solubility of BaSO4 in a solution
in which [H3O+] is 3.5 M. Ksp(BaSO4) = 1.1 x...