Solubility product of M(oh)3 and M(oh)2 are 10^-23 and 10^-14 . Which ...
B)).the solubility of M+2 is more than M+3 ion so precipitation occur first in M+3 ion
Solubility product of M(oh)3 and M(oh)2 are 10^-23 and 10^-14 . Which ...
Solubility Product and Precipitation
When a sparingly soluble salt is dissolved in water, it dissociates into its ions. The extent to which a salt will dissolve can be determined by its solubility product (Ksp) value. The solubility product is the product of the concentrations of the ions raised to the power of their stoichiometric coefficients in the balanced equation for the dissociation of the salt.
In this case, we are given the solubility product values for M(OH)3 and M(OH)2 as 10^-23 and 10^-14, respectively. Let's assume that M2+ and M3+ ions are present in the solution.
Precipitation of M(OH)3 and M(OH)2
When NH4OH is added to the solution, it will react with the M2+ and M3+ ions to form precipitates. The solubility of a compound is determined by comparing the value of its solubility product (Ksp) with the ion product (IP) of the solution.
The ion product (IP) is calculated by multiplying the concentrations of the ions in the solution raised to the power of their stoichiometric coefficients. If the ion product is greater than the solubility product, precipitation occurs.
Let's compare the ion product (IP) for M(OH)3 and M(OH)2 with their respective solubility products (Ksp).
Precipitation of M(OH)3:
The ion product for M(OH)3 can be represented as [M2+][OH-]^3. Since the concentration of OH- ions is determined by the concentration of NH4OH, which is in excess, we only need to consider the concentration of M2+ ions.
If the Ksp for M(OH)3 is 10^-23, and the concentration of M2+ ions exceeds the concentration given by the Ksp, precipitation of M(OH)3 will occur first.
Precipitation of M(OH)2:
The ion product for M(OH)2 can be represented as [M3+][OH-]^2. Again, since the concentration of OH- ions is determined by the concentration of NH4OH, we only need to consider the concentration of M3+ ions.
If the Ksp for M(OH)2 is 10^-14, and the concentration of M3+ ions exceeds the concentration given by the Ksp, precipitation of M(OH)2 will occur.
Conclusion:
Comparing the solubility product values, we see that the Ksp for M(OH)2 is higher than that of M(OH)3. Therefore, the precipitation of M(OH)2 will occur first when NH4OH is added to the solution containing M2+ and M3+ ions. The correct answer is option b) M3.
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