Hey guys so for this question I can't seem to understand why the molar solubility of MgSO4 would be irrelevant. I thought that eq reactions are reversible;
MgSO4 (s) <-> Mg2+ + SO42-
and so wouldn't the molar solubility of MgSO4 be important as well since it still has the possibility of precipitating? Thanks guys.
Item 32
Solution
When equal volumes of solutions of MgSO4 and NiF2 are mixed, a precipitate forms. Which of the following pieces of information will be LEAST useful in determining the identity of the precipitate?
A Molar solubility of MgF2
B Molar solubility of MgSO4
The examinee is asked to consider a situation in which two salts are each dissolved in a solvent to make two separate solutions, and then the two solutions are mixed. It is possible for the dissolved ions from each solution to then combine to form a precipitate. The likelihood of precipitate formation for a given cation/anion pair depends on that salts molar solubility: the greater the solubility, the greater the tendency for that salt to stay in solution. Alternately, a salt with a low molar solubility will have a greater tendency towards precipitation. Thus, the most important pieces of information are the solubilities of the salts that could form from the ions that encounter one another in the mixed solution. If magnesium cations from the first solution pair up with fluoride anions from the second solution, then a precipitate could form, depending on the molar solubility of that salt. Another combination is possible: the cation from the second solution, nickel(II), could combine to form a precipitate with the anion from the first solution, sulfate. So it would be useful to know the molar solubility of nickel(II) sulfate too. What is NOT needed is the molar solubility of the salts in the original solutions. Because they are in solution already and mixing them with an aqueous solution of a different solute cannot cause precipitate formation, their solubilities are irrelevant. Magnesium sulfate is the salt in the first solution, and knowing its molar solubility will not help answer the question about precipitates that might form once the solutions are mixed. Thus, option B is the best answer.
C Molar solubility of NiSO4
D Concentration of the NiF2 solution
MgSO4 (s) <-> Mg2+ + SO42-
and so wouldn't the molar solubility of MgSO4 be important as well since it still has the possibility of precipitating? Thanks guys.
Item 32
Solution
When equal volumes of solutions of MgSO4 and NiF2 are mixed, a precipitate forms. Which of the following pieces of information will be LEAST useful in determining the identity of the precipitate?
A Molar solubility of MgF2
B Molar solubility of MgSO4
The examinee is asked to consider a situation in which two salts are each dissolved in a solvent to make two separate solutions, and then the two solutions are mixed. It is possible for the dissolved ions from each solution to then combine to form a precipitate. The likelihood of precipitate formation for a given cation/anion pair depends on that salts molar solubility: the greater the solubility, the greater the tendency for that salt to stay in solution. Alternately, a salt with a low molar solubility will have a greater tendency towards precipitation. Thus, the most important pieces of information are the solubilities of the salts that could form from the ions that encounter one another in the mixed solution. If magnesium cations from the first solution pair up with fluoride anions from the second solution, then a precipitate could form, depending on the molar solubility of that salt. Another combination is possible: the cation from the second solution, nickel(II), could combine to form a precipitate with the anion from the first solution, sulfate. So it would be useful to know the molar solubility of nickel(II) sulfate too. What is NOT needed is the molar solubility of the salts in the original solutions. Because they are in solution already and mixing them with an aqueous solution of a different solute cannot cause precipitate formation, their solubilities are irrelevant. Magnesium sulfate is the salt in the first solution, and knowing its molar solubility will not help answer the question about precipitates that might form once the solutions are mixed. Thus, option B is the best answer.
C Molar solubility of NiSO4
D Concentration of the NiF2 solution