Consider the dissolution of MnS in water (Ksp = 3.0*10^-14)
MnS + H2O ----> Mn^2+ = HS- + OH-
How is the solubility of manganese(II) sulfide affected by the addition of aqueous 6M ammonia to the system?
a) the solubility with increase
b)the solubility will be unchanged
c)the solubility will decrease
d)can not be known without the K
e) the amount of ammonia added must be known before its effect can be predicted
I'm a little confused on this, so any help would be appreciated. Thanks:)
MnS + H2O ----> Mn^2+ = HS- + OH-
How is the solubility of manganese(II) sulfide affected by the addition of aqueous 6M ammonia to the system?
a) the solubility with increase
b)the solubility will be unchanged
c)the solubility will decrease
d)can not be known without the K
e) the amount of ammonia added must be known before its effect can be predicted
I'm a little confused on this, so any help would be appreciated. Thanks:)
-
Hello,
We know that if you add ammonia to water, it will produce NH4+ and OH-
Therefore, if we add it to the solution, it will increase the amount of product and the solubility will decrease because of an increased concentration of OH- in the solution. Because of a very low K value, the MnS can only dissolve to a certain amount and adding more of the product will cause solubility to decrease. C
We know that if you add ammonia to water, it will produce NH4+ and OH-
Therefore, if we add it to the solution, it will increase the amount of product and the solubility will decrease because of an increased concentration of OH- in the solution. Because of a very low K value, the MnS can only dissolve to a certain amount and adding more of the product will cause solubility to decrease. C