1. The molar solubility of magnesium carbonate in a 0.267 M ammonium carbonate solution is ______ M.
2. The molar solubility of silver phosphate in a 0.201 M silver nitrate solution is _____ M.
1) MgCO3 Mg2+(aq) + CO32-(aq)
let the solubility of MgCO3 is S mol/L
Thus, [Mg2+] = [CO32-] = S mol/L
Ammonium carbonate is a strong electrolyte which dissociates as,
(NH4)2CO3 2NH4+(aq) + CO32-
Thus, [CO32-] = 0.267 M
Hence, overall [CO32-] = ( S + 0.267 ) M or mol/L
Ksp = [Mg2+] [CO32-]
= S (S + 0.267)
or, 3.5 x 10-8 = S (S + 0.267) = S2 + 0.267 S
owing to the very small Ksp vale, S2 can be neglected
or, 3.5 x 10-8 = 0.267 S
or, S = 1.31 x 10-7 mol/L
Hence, the solubility of MgCO3 is 1.31 x 10-7 mol/L
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