I found thw ksp values for those listed, but not for silver hydroxide and im con

Question

I found thw ksp values for those listed, but not for silver hydroxide and im confused how to go on with this problem

Consider these compounds: A. Ag2Cro B. Mg(OH)2 C. MnS D. MgCO3 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that silver hydroxide is more soluble than, and silver hydroxide is less soluble than It is not possible to determine whether silver hydroxide is more or less soluble than by simply comparing Ksp values.

Explanation / Answer

Hi, I recommend you the Lange's Handbook of Chemistry, there I found the Ksp of AgOH that is 2 x 10-8

You can only compare the solubility with the Ksp of compounds with the same stoichiometry, this is because at equilibrium (to calculate the solubility of the compound) you consider the stoichiometric coefficients, for different stoichiometry the numbers change and aren't comparable. For example:

AgOH ----> Ag+ + OH- (Reaction to compare, 1 reactant and 2 products)

MgCO3 ---> Mg2+ + CO32- (Comparable reaction, 1 reactant and 2 products, same stoichiometry)

Ag2CrO4 ---> 2 Ag+ + CrO42- (Incomparable reaction, 1 reactant and 3 products, different stoichiometry)

As the Ksp is bigger the compound is more soluble and we can use this to compare.

The answer of the exercise is:

The silver hydroxide is more soluble than MnS (C), and silver hydroxide is less soluble than MgCO3 (D) . It is not possible to determine whether silver hydroxide is more or less soluble than Ag2CrO4 (A) and Mg(OH)2 (B) by simply comparing Ksp values.

Compound Ksp AgOH 2 x 10-8 Ag2CrO4 1.12 x 10-12 Mg(OH)2 5.61 x 10-12 MnS 2.5 x 10-10 amorfous , 2.5 x 10-13 cristalline MgCO3 6.82 x 10-6

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