Question

Rank the solubilities of the following salts, shown with their Ksp values at 25°C in order of increasing solubility, i.e. least soluble = 1 and most soluble = 3. Ag2CO3 Ksp = 8.1 x 10^-12 Mn(OH)2 Ksp = 2.0 x 10^-13 CdCO3 Ksp = 5.2 x 10^-12 You can not simply compare the Ksp values if there are different numbers of ions formed in solution. Write out the equilibrium reaction: AaBb(s) ? a A (aq) + b B (aq) Write out the equilibrium expression: Ksp = [aA]^a[bB]^b and solve for the equilibrium concentration of one of the species. Based on the stoichiometry, this will tell you how much of the solid will dissolve.

          Rank the solubilities of the following salts, shown with their Ksp values at 25°C in order of increasing solubility, i.e. least soluble = 1 and most soluble = 3.
Ag2CO3 Ksp = 8.1 x 10^-12
Mn(OH)2 Ksp = 2.0 x 10^-13
CdCO3 Ksp = 5.2 x 10^-12
You can not simply compare the Ksp values if there are different numbers of ions formed in solution.
Write out the equilibrium reaction: AaBb(s) ? a A (aq) + b B (aq)
Write out the equilibrium expression:
Ksp = [aA]^a[bB]^b
and solve for the equilibrium concentration of one of the species.
Based on the stoichiometry, this will tell you how much of the solid will dissolve.

Rank the solubilities of the following salts, shown with their Ksp values at 25°C in order of increasing solubility, i.e. least soluble = 1 and most soluble = 3.
Ag2CO3 Ksp = 8.1 x 10^-12
Mn(OH)2 Ksp = 2.0 x 10^-13
CdCO3 Ksp = 5.2 x 10^-12
You can not simply compare the Ksp values if there are different numbers of ions formed in solution.
Write out the equilibrium reaction: AaBb(s) ? a A (aq) + b B (aq)
Write out the equilibrium expression:
Ksp = [aA]^a[bB]^b
and solve for the equilibrium concentration of one of the species.
Based on the stoichiometry, this will tell you how much of the solid will dissolve.

Added by Gary B.

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