What is the concentration of gold ion in a saturated solution of Aucl_3, if the

Question

What is the concentration of gold ion in a saturated solution of Aucl_3, if the Ksp is 2.9 times 10^-23 at a given temperature? What pH is required to prevent cloudiness (the formation of a precipitate) in a solution of 0.005 M V(NO_3)_3 if the ksp of V(OH)_3 is 4 times 10^-35? What is the mass (in g) of silver chromate (MW = 331.7 g/mol) that can dissolve in 1.00 L of 0.10 M AgNO_3 solution? The solubility product for Ag_2CrO_4: K_sp = 1.2 times 10^-12 Will a precipitate from in a solution of 0.0025 M Nicl_2 if the pH is adjusted to 3.2?(The Ksp of Ni(OH)_2 is 5.5 times 10^-16) Justify your answer mathematically. How much silver is deposited and at which electrode in the reaction Ag^+ + 1e^- rightarrow Ag, if electrolysis is allowed to occur for 6 hours with a steady current of 2.5 amps.

Explanation / Answer

C)

AuCl3   ---------------> Au+3   + 3 Cl-

                                      S             3S

Ksp = [Au+3][Cl-]^3

2.9 x 10^-23 = S x (3S)^3

2.9 x 10^-23 = 27S^4

S = 1.02 x 10^-6 M

concentration of gold ion = 1.02 x 10^-6 M

2)

V(OH)3   -------------> V+3   +   3 OH-

                                  0.005       3 S

Ksp = [V+3][OH-]^3

4 x 10^-35 = 0.005 x [3S]^3

[OH-] = 2 x 10^-11

pOH = -log (2 x 10^-11)

pOH = 11

pH = 3.00

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