The Ksp of Fe3(PO4)2 is 2.22⋅10^−25 M. Calculate the solubility of each ion in a saturated solution:       (??) M Fe2+    (??) M PO43-

If a solution contained Ni2+ ions at a concentration of 0.1 M, what pH would have to be reached toprecipitate 99% of the Ni2+ as Ni(OH)2?

A 0.100 L solution of 0.250 M AgNO30.250 M AgNO3 is combined with a 0.100 L solution of 1.00 M Na3PO4.1.00 M Na3⁢PO4. Calculate the concentration of Ag+Ag+ and PO3−4PO43− at equilibrium after the precipitation of Ag3PO4Ag3⁢PO4 (?sp=8.89×10−17).

The iodate ion has a number of insoluble compounds. The Ksp for AgIO₃ is 3.0 x 10⁻⁸ and the Ksp for La(IO₃)₃ is 7.5 x 10⁻¹². What is the solubility of AgIO₃ in a 0.200 M solution of NaIO3?

-18 A solution contains 4.0 x 10-6 M Na3PO4. What is the minimum concentration of AGNO3 that would cause precipitation of solid Ag, PO4 (Ksp = 1.8 × 10)? Concentration 3.32х10^-5 M

The iodate ion has a number of insoluble compounds. The Ksp for AgIO₃ is 3.0 x 10⁻⁸ and the Ksp for La(IO₃)₃ is 7.5 x 10⁻¹². a)What is the solubility of AgIO₃ in a 0.260 M solution of NaIO₃? b) What is the solubility of La(IO₃)₃ in a 0.260 solution of NaIO₃ c) Which compound is more soluble

The pK₂ value for H₂S is 7.00. What mole ratio of KHS to H₂S is needed to prepare a buffer with a pH of 7.27? [HS] [H₂S]

The iodate ion has a number of insoluble compounds. The Ksp for AgIO₃ is 3.0 x 10⁻⁸ and the Ksp for La(IO₃)₃ is 7.5 x 10⁻¹². What is the solubility of La(IO₃)₃ in a 0.115 M solution of NaIO₃?

What is the pH of a saturated solution of Mn(OH)₂? (Ksp for Mn(OH)₂ = 1.6 × 10-1³).

Jj.49.