Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn2+, Zn2+, Pb2+ and Cu2+ and 0.10 M in H,S at a pH of 1.0? Metal Sulfide MnS Zns 3x> Pbs Cus Top to bottom, Ksp values are; 3x 1016, 3x 102-, 3x 107-, 6x 1016-. PbS, Cus Cus MnS ZnS, PbS, CuS

Find the pH value for a solution containing 0.5 mg/L of copper ion (Cu2+) dissociated from Cu(OH)2 at equilibrium. If the pH of this solution is adjusted to 6 and 10, what would be the concentrations of copper ion in mg/L at equilibrium, respectively?

Jj.49.

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in the salt solution with a solution containing a common ion. Cd(OH)2(s) in a solution buffered at a pH of 10.995

How many grams of (CH3)NHCI (FW 95.5) needs to be dissolved in a 0.1 Lof 0.5 M (CH3)N (Kb = 6.3 x 10-5) to achieve a buffered solution with a pH of 9? O 51.4 g O None of these are correct. O 34.7 g O 44.9 g

Write a balanced net ionic equation to show why the solubility of AgCN(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Be sure to specify states such as (aq) or (s). K= + + +

A solution is known to contain 0.0150 M Ce(SO4)32-. When 25 ml of this solution is titrated, 23.44 mL of 0.032 M FeSO4 solution is required to reach the equivalence point. The reaction of the two substances produces Fe3+ as one of the products. Determine the oxidation number of Ce after the reaction.