Silver carbonate, Ag2CO3, is a sparingly soluble solid. A saturated solution is prepared by placing solid silver carbonate in pure water in which the silver ion concentration, [Ag1+], was found to be 1.02E-04 M.
a. What is the concentration of carbonate ions, [CO32-]?
b. What is the molar solubility of silver carbonate, Ag2CO3?
c. What is the solubility product constant, Ksp, for silver carbonate, Ag2CO3?
2007-11-06 06:10:12 · 3 answers · asked by Nick P 1 in Science & Mathematics ➔ Chemistry
As for every 2 mol of Ag+ you have 1 mol of (CO3)2- you will have (1.02E-4 / 2 )mol/l Carbonate ions
the same reasoning will leads to the answer to b for 2 mol of Ag+ there is 1 mole of Ag2CO3 solubility : (1.02E-4 / 2 )mol/l
K= [c((CO3)2-)*c^2(Ag+)]
calculate the numbers for yorself
2007-11-06 06:20:51 · answer #1 · answered by klimbim 4 · 0⤊ 0⤋
Ag2CO3 <===> 2Ag+ + CO3=
a. 0.5 x (1.02 x 10^-4) = 0.50 x 10^-4 = 5 x 10^-5 mole/L
b. 5 x 10^-5 mole/L
c. Ksp = [Ag+]^2[CO3=] = (1.02x10^-4)^2(5x10^-5) = 5.2 x 10^-13
2007-11-06 14:22:49 · answer #2 · answered by steve_geo1 7 · 0⤊ 0⤋
a.) half the silver conc. = 0.51E-4 M = 5.1E-5M
b.) again , half that of silver, 5.1E-5M
c.) (1.02E-4)^2 x (5.1E-5) = 5.3 E-13 (mole/L)^3
2007-11-06 14:19:12 · answer #3 · answered by ferrous lad 4 · 0⤊ 0⤋