1) At a certain temperature the K sp of Ag 2 SO 4 is 1.06 x 10 -5 . What is the
ID: 1018588 • Letter: 1
Question
1) At a certain temperature the Ksp of Ag2SO4 is 1.06 x 10-5. What is the molar soliubility of silver sulfate in water in units of M (mol/liter).
Express your answer in scientific notation.
2) The Ksp of BaCO3 is 5.0 x 10-9. What is the soliubility of barium carbonate in a solution that contains 1.67 M of Na2CO3?
3) Based on the acid/base properties of the salt, do you expect each of the following to be more soluble in acid, more soluble in base, or no effect of pH on solubility?
- CaSO4 A. More soluble in basic solutions
- NH4Cl B. More soluble in acidic solutions
- KBr C. Little or no effect of pH on solubility
- BaCO3
Explanation / Answer
) At a certain temperature the Ksp of Ag2SO4 is 1.06 x 10-5. What is the molar soliubility of silver sulfate in water in units of M (mol/liter).
Solubility in water.
If x moles of solid Ag2SO4 dissolves 2x moles of Ag^+ and x moles of SO4^2- ions are formed.
Given that; the Ksp of Ag2SO4 is 1.06 x 10-5
Ag2SO4 = 2Ag+ + SO42-
Assume that the solubility is S.
Ksp = (2x)^2(x) = 1.06 x 10^-5
4x^3 = 1.06 x 10^-5
x^3 = 2.65x 10^-6
X=0.0138 M or 1.38*10^-2 mol/L is the solubility of salt in water
2) The Ksp of BaCO3 is 5.0 x 10-9. What is the soliubility of barium carbonate in a solution that contains 1.67 M of Na2CO3?
BaCO3 <------> Ba2+ + CO32-
at equilibrium
[Ca2+]= x
[CO32-] = x + 1.67
5.0 x 10^-9 = (x)( x+ 1.67 )
use quadratic equation
5.0 x 10^-9 = X^2 + 1.67X
X^2 + 1.67X - 5.0 x 10^-9
x = molar solubility = 2.994 M
3) Based on the acid/base properties of the salt, do you expect each of the following to be more soluble in acid, more soluble in base, or no effect of pH on solubility?
- CaSO4 More soluble in acidic solutions
NH4Cl More soluble in basic solutions
BaCO More soluble in acidic solutions
KBr Little or no effect of pH on solubility