What is the [H_3O^+] in each of these final solutions (after dilution and before
ID: 538817 • Letter: W
Question
What is the [H_3O^+] in each of these final solutions (after dilution and before any reaction occurs)? ______ SAVE everything and record your observations as the reactions proceed. Check page 153 to make sure that any solid (or cloudiness) that formed corresponds to the sulfide of the cation being tested. Which solution(s) did not give a precipitate? Fe, 2n Which solution(s) did not give the expected precipitate? Ag, Cu Would substituting 1 M HCl for the 1 M H_2SO_4 make a difference in any of your observations above? Why? yes b/c SO_4^2- reacts differently than Cl^- blc of its charge. Would you expect any change to be observed if 2 mL of 5% TAA solution and 1 mL of 1 M H_2S0_4 were heated with 0.1 M solutions of Ca^2+, Mg(H_20)_6^2+, or Al(H_20)_5^3+? ______ Use your acid/base table to predict the result of treating a 1 M NH_3 solution with H_2S gas. The rxn would go to a small extent b/c H_2S NH_3 have relative strengths. Consider treating both pure water and 1 M NaOH with H_2S gas. How will [HS^-] in each of these solutions compare with [HS^-] in the solution of 1 M NH_3 and H_2S? _______Explanation / Answer
Cation analysis
From the given list of cations,
substituting the system with 1 M H2SO4 instead of 1 M HCl would result in different results as the acidity of the solution would now be greater than the one before.
When heated with 1 M H2SO4, Ca2+ forms CaSO4 precipitate as insoluble salt and MgSO4 and Al2(SO4)3 are soluble salts.
Reaction of 1 M NH3 with H2S produce (NH4)2S.
NH3 is a base which abstracts proton from H2S and thus it is an acid-base reaction to form salt (NH4)2S as the net product of the reaction.
1 M NaOH is a strong base and it would react completely with H2S in solution to give HS- species as the product. Whereas, in water, H2S a weak acid would disscoiate only to an small extent and thus concentration of H2S would be very low.
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