Question

Having a tough time.

1. What is the molar solubility of Mg3(PO4)2 in a 0.860 M solution of sodium phosphate? The Ksp for Mg3(PO4)2 = 1.04 x 10-24 M 2. What is the molar solubility of Ag2SO4 in a 0.950 M solution of Al2(SO4)3? The Ksp for Ag2SO4 = 1.20 x 10-5 1.33e-5 x M 3. Select all of the following that are true about the common ion effect for dissolving solids. If you add potassium sulfate to a saturated solution of PbSO4, more precipitate will form. The addition of a soluble salt containing a common ion will decrease the solubility of a sparingly soluble salt. Mg3(PO4)2 will be more soluble in a 1.0 M solution of magnesium nitrate than in a 1.0 M solution of magnesium sulfate. The common ion effect only works when adding anions. CaCO3 can be made more soluble by adding a soluble source of Ca2+ ion. AgBr is more soluble in a 1.0 M solution of sodium bromide than it is in a 1.0 M solution of calcium bromide.

Answer 1

3) 1 & 2 & 3 &6 are correct

3- mg (pon) - 3 mght + 2 pour 38 (28+0.80) kop - (32) ? ( 23 + 0.86)? - 1.04x1024 As Kop is very less, 23 + 0.86 0.86 (33)3(0.86% = 1.04x1024 s = [ 3.73x169M & 3.73e-9 Ag sou 2 Ag+ + soa 25 s +2.85 (29)*(3+9.85)= 1.20x105 Ts= 103 1-3 m