Propose a separation scheme to separate Ag^+ from a solution containing Fe^2+ an
ID: 1019878 • Letter: P
Question
Propose a separation scheme to separate Ag^+ from a solution containing Fe^2+ and Sn^4+. Use lessthanorequalto Chatlier's principle to predict what will happen to S^2- in the following equation when the pH is decreased. H_2S (aq) + 2 H_2O(l) 2 H_3O^+ (aq) + S^2- (aq) If the application of heat causes a reaction to produce more products, is the reaction endothermic or exothermic? What is the net ionic equation when Cu(NO_3)_2(aq) reacts with H_2S(aq) A student has a yellow reside that is either SnS_2 or CdS. What could be add confirm the identity of the precipitate? A student carries out a separation scheme starting with Bi^3+, Cd^2+ and Cu^2+. At the end of the experiment, the student has blue Bi(OH)_3 solid instead of white. What is likely the problem? A solution contains either Ba^2+ or Ca^2+. What test could be used to determine the identity of the cation? What is true about the Group IV hydroxides compared to the Group III hydroxides?Explanation / Answer
Q.1: Add 6M HCl to the solution. Ag+(aq) (Group A cation) will be precipitated as AgCl(s) and rest of the cations will remain in the solution. Now separate the precipitate containing Ag+(aq).
Q.2: When we decrease the pH, the cncentration of H3O+(aq) also dereases. Now according to Le-chatelier's principle, in order to increase the concentration of H3O+(aq), more and more H2S reacts with H2O to form H3O+(aq) and S2-. Hence the concentration of S2- increases. (answer)
Q.3: Since an endothermic reaction requires heat, application of heat causes a reaction to produce more product in case of endothermic reaction. Hence the reaction is endothermic.
Q.4: Net ionic equation: Cu2+(aq) + S2-(aq) ------ > CuS (s)
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