The solubility of silver carbonate (mm = 275.745), is 33.5 mg/L. What is its mol

Question

The solubility of silver carbonate (mm = 275.745), is 33.5 mg/L. What is its molar solubility, and what is its K_sp? A student preforming the lab for the solubility of calcium iodate, titrated a 10.00 mL sample of saturated calcium iodate solution with a 0.011 M sodium thiosulfate solution. The titration required 21.62 mL to turn the solution clear. What was the concentration of the iodate in the solution? What was the K_sp that the student determined for that titration? (Consult the background section).

Explanation / Answer

1)

molar mass of Ag2CO3 = 275.7 g/mol

s = 33.5 mg/L

= 0.0335 g/L

= 0.0335/275.7 mol/L

= 1.215*10^-4 M

Answer: 1.215*10^-4 M

Ag2CO3   <—> 2Ag+       +   CO32-

           2s           s

Ksp = [Ag+]^2 [CO32-]

Ksp = (2s)^2 * s

Ksp = 4*s^3

= 4*(1.215*10^-4)^3

= 7.18*10^-12

Answer: Ksp is 7.18*10^-12

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