Solubility and Equilibrium
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AP Chemistry › Solubility and Equilibrium
Calculate the molar solubility of AgBr in 0.050 M AgNO3 at room temperature. The Ksp of AgBr is 5.4 x 10-13.
1.08 x 10-11 M
2.16 x 10-11 M
1.08 M
2.16 M
1.57 x 10-12 M
Explanation
Would the molar solubility of Cr(OH)3 increase or decrease as the pH is lowered (i.e. made more acidic)?
Increase
Decrease
There is no change
Can not be determined
Explanation
Since Cr(OH)3 is a basic salt, decreasing the pH makes it more soluble.
Calculate the molar solubility of SrF2 in 0.023M NaF. The Ksp for SrF2 is 4.3 x 10-9.
3.2 x 10-3 M
1.6 x 10-3 M
8.1 x 10-6 M
3.2 x 10-5 M
5.2 x 10-4 M
Explanation
Calculate the molar solubility of Mn(OH)2 at pH 9.5. The Ksp for Mn(OH)2 is 1.6 x 10-13.
1.5 x 10-3 M
2.4 x 10-3 M
3.5 x 10-4 M
1.6 x 10-4 M
2.1 x 10-5 M
Explanation
Calculate the molar solubility of CaF2 (Ksp = 3.9 x 10-11) in a room temperature solution of 0.010 M Ca(C2H3O2)2.
1.6 x 10-2 M
3.2 x 10-2 M
4.2 x 10-4M
3.7 x 10-4 M
3.1 x 10-5 M
